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Worksheets

HS Chemisty - Final Overview

Total questions: 170

Worksheet time: 1hrs 26mins

Name
Class
Date
1.

What are the two types of properties of matter?

a)
Thermal properties and electrical properties
b)

Extensive properties and Intensive properties

c)
Biological properties and physical properties
d)
Solid properties and liquid properties
2.

How do you calculate Electron Domains?

a)
Count only the bonding pairs around the central atom.
b)
Multiply the number of atoms by the number of bonds.
c)

Add the number of lone pairs and bonding pairs around the central atom.

d)
Add the atomic numbers of the surrounding elements.
3.

What is the biggest impact that lone pairs have on the structure of a molecule?

a)
Lone pairs increase the number of bonds in a molecule.
b)
Lone pairs have no effect on molecular shape.
c)

Lone pairs cause the molecule to be asymmetrical

d)
Lone pairs only affect the color of the molecule.
4.

What are the qualifications for a molecule's shape to be linear?

a)

Two electron domains and no lone pairs on the central atom.

b)
Two bonding pairs and one lone pair on the central atom.
c)
One bonding pair and one lone pair on the central atom.
d)
Three bonding pairs and no lone pairs on the central atom.
5.

What are the qualifications for a molecule's shape to be bent?

a)

A molecule's shape is bent if it has either three electron domains, one of which is a lone pair, or it has four electron domains, two of which are lone pairs.

b)
A molecule's shape is bent if it has two bonded atoms and two lone pairs on the central atom.
c)
A molecule's shape is bent if it has three bonded atoms and no lone pairs.
d)
A molecule's shape is bent if it has one bonded atom and one lone pair on the central atom.
6.

What are the qualifications for a molecule's shape to be trigonal planar?

a)
Two bonding pairs and one lone pair around the central atom.
b)
Four bonding pairs and no lone pairs around the central atom.
c)
Three bonding pairs and one lone pair around the central atom.
d)

Three electron domains including no lone pairs around the central atom.

7.

What are the qualifications for a molecule's shape to be trigonal pyramidal?

a)

Four electron domains, one of which is a lone pair.

b)
Five regions of electron density, four bonding pairs, one lone pair.
c)
Two regions of electron density, two bonding pairs, two lone pairs.
d)
Three regions of electron density, two bonding pairs, one lone pair.
8.

What are the qualifications for a molecule's shape to be tetrahedral?

a)
Three bonded atoms/groups around a central atom with sp2 hybridization.
b)
Four lone pairs around a central atom with sp3 hybridization.
c)
Two bonded atoms/groups around a central atom with sp hybridization.
d)

Four electron domains, none of which are lone pairs.

9.

What are the qualifications for a molecule's molecular polarity to be polar?

a)

A molecule is polar if it is linear (w different electronegativity), bent, or trigonal pyramidal.

b)
A molecule is polar if it has a high molecular weight.
c)
A molecule is polar if it has only nonpolar bonds.
d)
A molecule is polar if it has a symmetrical shape and no polar bonds.
10.

What are the qualifications for a molecule's molecular polarity to be non-polar?

a)

A molecule is non-polar if it is linear (w similar electronegativity), trigonal planar, or tetrahedral.

b)
A molecule is non-polar if it contains only polar bonds.
c)
A molecule is non-polar if it has a high electronegativity difference between atoms.
d)
A molecule is non-polar if it has a linear shape and unequal distribution of charge.
11.

What is the law of conservation of mass?

a)
Mass can be created in chemical reactions.
b)
Mass is conserved in chemical reactions; it cannot be created or destroyed.
c)
Mass is lost during combustion reactions.
d)
Mass is only conserved in physical changes.
12.

What are the main three rules to follow when balancing a chemical equation?

a)

1) Count atoms, 2) Adjust coefficients (never subscripts), 3) Simplify ratios.

b)
Combine elements before balancing
c)
Ignore the number of atoms
d)
Use equal signs for reactions
13.

How would you find the number of atoms of an element in a chemical equation?

a)

Multiply the coefficients and subscripts in the chemical formula.

b)
Use the periodic table to estimate the number of atoms.
c)
Add the atomic numbers of the elements together.
d)
Multiply the coefficients by the atomic mass.
14.

What are the 5 types of chemical reactions?

a)
Oxidation, Reduction, Hydrolysis, Precipitation, Neutralization
b)
Sublimation, Crystallization, Distillation, Filtration, Evaporation
c)
Electrolysis, Polymerization, Fermentation, Condensation, Hydrolysis
d)
Synthesis, Decomposition, Single Replacement, Double Replacement, Combustion
15.

What are the two products formed in all combustion reactions?

a)
Hydrogen and sulfur
b)
Methane and ammonia
c)
Oxygen and nitrogen
d)
Carbon dioxide and water
16.

Why is acid rain created? What is the reasoning behind its' creation?

a)
Acid rain forms when rainwater evaporates and leaves behind minerals.
b)
Acid rain is caused by volcanic eruptions releasing carbon dioxide.
c)

Acid rain is created through the combustion of amino acids and proteins in organic matter.

d)
Acid rain is a result of natural processes like plant respiration.
17.

What are intermolecular forces (IMF)?

a)
Intermolecular forces are the same as chemical bonds.
b)
Intermolecular forces are only present in solids.
c)

Intermolecular forces (IMF) are weak electrostatic interactions (forces) between molecules.

d)
IMF are the forces that hold atoms together in a molecule.
18.

What are the 5 main types of IMFs?

a)
Covalent bonds
b)
Metallic bonds
c)
Van der Waals forces
d)

London dispersion forces, Dipole-dipole interactions, Hydrogen bonding, Ion-dipole interactions, Dipole induced dipole interactions

19.

What are the qualifications for polar molecules? What IMFs can they form?

a)

Polar molecules have 6 or less carbon chains with O or N; can form hydrogen bonds, dipole-dipole interactions, and London dispersion forces.

b)
Polar molecules can only form covalent bonds.
c)
Polar molecules do not interact with nonpolar molecules.
d)
Polar molecules can only form ionic bonds.
20.

What are the qualifications for non-polar molecules? What IMFs can they form?

a)
Non-polar molecules have a strong permanent dipole moment.
b)
Non-polar molecules can only form hydrogen bonds.
c)
Non-polar molecules cannot form any intermolecular forces.
d)

Non-polar molecules have no O or N if organic; can form London Dispersion forces.

21.

What are dipoles?

a)
Dipoles are single charges with no opposite counterpart.
b)
Dipoles are only found in magnetic materials.
c)
Dipoles are always stationary and do not move.
d)

Dipoles are a type of electrostatic interaction that are created by a separation of charge which is created by a gap in electronegativity of atoms; is asymmetrical.

22.

What do f, k, q1, q2, and r stand for in Coulomb's law?

a)

f = attractive force; k = constant; q1 = effective nuclear charge; q2 = any valance electron; r = radius

b)
f = (q1 + q2) / (k * r^2)
c)
f = k * (q1 * q2) * r^2
d)
f = k * (q1 + q2) / r
23.

A stronger attractive force is associated with the size of the atom in what way?

a)
Smaller atoms have stronger attractive forces due to higher effective nuclear charge.
b)
Larger atoms have stronger attractive forces due to lower effective nuclear charge.
c)
Smaller atoms have weaker attractive forces due to increased electron shielding.
d)
Atoms of all sizes have equal attractive forces regardless of size.
24.

What is effective nuclear charge?

a)
Effective nuclear charge is the net positive charge experienced by an electron in an atom.
b)
Effective nuclear charge is the charge of an electron in isolation.
c)
Effective nuclear charge is the force that holds the nucleus together.
d)
Effective nuclear charge is the total charge of the nucleus.
25.

What is the trend with distance and effective nuclear charge (q1) across a period?

a)
Effective nuclear charge decreases across a period.
b)
Effective nuclear charge remains constant across a period.
c)

Distance increases; Effective nuclear charge fluctuates randomly across a period.

d)

Distance stays relatively the same; effective nuclear charge increases across a period (left to right).

26.

Why does reactivity increase down a period and right to left across a period?

a)

Reactivity increases since the attractive force decreases due to increased size or lower effective nuclear charge.

b)
Reactivity increases down a group and remains constant across a period.
c)
Reactivity remains constant down a group and increases from left to right across a period.
d)
Reactivity decreases down a group and from left to right across a period.
27.

What is metallic character?

a)
Metallic character refers to the ability of an element to form covalent bonds.
b)

Metallic character is ability of metals to lose electrons (their chemical reactivity).

c)
Metallic character is the measure of an element's non-metallic properties.
d)
Metallic character is the tendency of an element to be a gas at room temperature.
28.

What is Ionization Energy?

a)

Ionization energy is the energy needed to remove an electron from an atom (for metals).

b)
Ionization energy is the mass of an electron in an atom.
c)
Ionization energy is the temperature at which an atom becomes ionized.
d)
Ionization energy is the energy released when an electron is added to an atom.
29.

What is the trend for ionization energy in a group and a period?

a)
Ionization energy increases down a group and decreases across a period.
b)
Ionization energy decreases across a period and increases down a group.
c)
Ionization energy remains constant across a period and a group.
d)

Ionization energy increases across a period and decreases down a group.

30.

What is electronegativity?

a)
Electronegativity refers to the temperature at which a substance melts.
b)
Electronegativity is the ability of an atom to attract electrons in a chemical bond.
c)
Electronegativity is the measure of an atom's size.
d)
Electronegativity is the speed at which electrons move in an atom.
31.

What is the shielding effect?

a)
The shielding effect is the increase of effective nuclear charge on outer electrons.
b)
The shielding effect refers to the attraction between electrons of the same energy level.
c)

The shielding effect is the effect of diminishing the attractive force that the VEs feel from the nuclear charge by CEs canceling out protons (as barriers).

d)
The shielding effect is the phenomenon where outer electrons gain energy from inner electrons.
32.

What are the trends for size and q1?

a)

Size tends to increase; q1 stays the same due to the shielding effect

b)
Size fluctuates randomly in q1 without any pattern.
c)
Size remains constant in q1 regardless of demand.
d)
Size decreases in q1 due to increased competition.
33.

What impacts the amount of energy needed for electrons to jump from lower to higher energy levels?

a)
The color of the light used in the experiment.
b)
The temperature of the surrounding environment.
c)

The strength of the force between the nucleus and electrons

d)
The mass of the electrons involved.
34.

What are the two equations for the speed of light?

a)
c = 3.00 x 10^8 m/s
b)
c = 1.5 x 10^8 m/s
c)

c = λν and λu

d)

c = hf

35.

What are the equations for frequency (f or u)?

a)

f = # wavelengths/time and f = c/ λ and 1/sec

b)
f = 2π/T
c)
f = λ/T
d)
f = T/v
36.

What are the equations for energy?

a)
P = IV
b)
F = ma
c)
W = Fd
d)

E = hu and hc/ λ

37.

What does v, u, h, and λ stand for?

a)

v = velocity, u = frequency, h = Planck's constant, λ = wavelength

b)
v: volume, u: uniformity, h: humidity, λ: luminescence
c)
v: vector, u: unit, h: harmonic, λ: length
d)
v: velocity, u: upward velocity, h: horizontal distance, λ: light frequency
38.

What are the 6 period trends or periodicity?

a)
1. Atomic Radius 2. Ionization Energy 3. Electronegativity 4. Electron Affinity 5. Metallic Character 6. Reactivity
b)
Atomic Mass
c)
Density
d)
Melting Point
39.

What is coulomb's law?

a)

Coulomb's law states that F = k[(Q1 x Q2) / r^2]

b)
Coulomb's law states that the force is constant regardless of distance.
c)
Coulomb's law describes the relationship between temperature and pressure.
d)
Coulomb's law applies only to magnetic charges.
40.

What is the difference between and Extensive and Intensive Property?

a)
Intensive properties depend on the type of material, while extensive properties do not.
b)
Extensive properties vary with the quantity of material, while intensive properties remain constant regardless of the amount.
c)
Extensive properties are always constant, while intensive properties vary with quantity.
d)
Both extensive and intensive properties are independent of the amount of material.
41.

What are some examples of Extensive and Intensive properties?

a)

Extensive: Weight, volume, mass

b)

Intensive: Weight, volume, mass

c)

Intensive: Density, temperature, boiling point, heat capacity

d)

Extensive: Density, temperature, boiling point, heat capacity

42.

What is true about the composition of the universe?

a)
The universe is made entirely of stars and planets.
b)

The universe is composed of dark energy (majority), dark matter, and ordinary matter.

c)
The universe is composed of gases and liquids.
d)
The universe consists only of black holes and neutron stars.
43.

What is the equation for density?

a)
Density = Mass / Volume
b)
Density = Mass + Volume
c)
Density = Volume / Mass
d)
Density = Mass x Volume
44.

What is the coorelation between density and slope of a line?

a)

The higher the slope = the higher the density

b)
The slope of a line has no relation to density or volume.
c)

The higher the slope = the lower the density

d)
The slope of a line is always zero regardless of density.
45.

What are the four unifying themes?

a)
Habitat destruction, Climate change, Pollution
b)
Species extinction, Genetic modification, Overfishing
c)

Natural selection, Symbiosis, Habitat fragmentation, Deforestation

d)

Structure determines function, energy is the driving force in nature, nature favors the lowest energy state, and nature favors diversity & complexity

46.

What is the Ground State?

a)

The lowest energy state; when electrons occupy the lowest energy rings (closest to the nucleus).

b)
The highest energy state of a quantum mechanical system.
c)
The average energy state of a quantum mechanical system.
d)
A state with no energy at all.
47.

How many electrons must occupy each energy level before another one can have electrons?

a)
2 electrons for the first level, 8 for the second level.
b)
2 electrons for the first level, 10 for the second level.
c)
3 electrons for the first level, 6 for the second level.
d)
1 electron for the first level, 4 for the second level.
48.

When an electron moves from a high energy level to a low energy level what happens? What happens in the reverse?

a)
An electron releases energy when moving to a higher energy level.
b)

Releases energy; uses energy.

c)
An electron does not change energy levels when moving between them.
d)
An electron gains energy when moving to a lower energy level.
49.

What commonly cause electrons to jump to higher energy levels?

a)
Absorption of sound waves
b)
Absorption of energy (heat, light, or electrical energy)
c)
Release of electrons from a magnetic field
d)
Cooling of the atom's environment
50.

What is the structure, IMF strength, and kinetic energy speed of a solid?

a)

Highly organized, very strong, very slow

b)

Intermediate, intermediate, intermediate

c)

Disorderly, very weak, very fast

51.

What is the structure, IMF strength, and kinetic energy speed of a liquid?

a)

Highly organized, very strong, very slow

b)

Intermediate, intermediate, intermediate

c)

Disorderly, very weak, very fast

52.

What is the structure, IMF strength, and kinetic energy speed of a gas?

a)

Highly organized, very strong, very slow

b)

Intermediate, intermediate, intermediate

c)

Disorder, very weak, very fast

53.

What are the 5 states on a heating curve that is endothermic?

a)
Solid, Liquid, Vapor, Sublimation, Gas
b)
Solid, Liquid, Gas, Plasma, Superfluid
c)
Solid, Melting, Liquid, Boiling, Gas
d)
Solid, Freezing, Liquid, Condensing, Plasma
54.

What are the 5 states on a heating curve when it is exothermic?

a)
Gas, Liquid, Freezing, Solid, Deposition
b)
Gas, Condensation, Liquid, Freezing, Solid
c)
Gas, Sublimation, Liquid, Melting, Solid
d)
Gas, Vaporization, Liquid, Boiling, Solid
55.

Why does the temperature remain the same during states 2 and 4 on a heating curve?

a)
The temperature increases as the substance absorbs heat.
b)
The temperature decreases due to energy loss during phase changes.
c)

The temperature stays the same for no apparent reason.

d)

The temperature remains the same since the energy is being used to break IMFs

56.

What is the difference between a pure substance and a mixture?

a)

A pure substance has a fixed composition (one thing); a mixture has variable composition.

b)
A pure substance is always a solid; a mixture can be a liquid or gas.
c)
A pure substance can be separated into its components; a mixture cannot.
d)
A pure substance has varying properties; a mixture has uniform properties.
57.

What is the difference between elements and compounds?

a)
Elements can be made of multiple types of atoms; compounds cannot.
b)
Compounds are always gases; elements are always solids.
c)
Elements are mixtures of different substances; compounds are pure substances.
d)
Elements consist of one type of atom; compounds consist of two or more types of atoms.
58.

What does it mean for something to be diatomic?

a)
Diatomic means consisting of three atoms.
b)
Diatomic refers to a single atom.
c)
Diatomic indicates a molecule with no atoms.
d)

Diatomic means consisting of two atoms

59.

What is the difference between homogenous and heterogenous?

a)
Homogeneous means varying composition; heterogeneous means consistent composition.
b)
Homogeneous means uniform composition; heterogeneous means non-uniform composition.
c)
Heterogeneous means all parts are identical.
d)
Homogeneous refers to a mixture of different substances.
60.

Where are electrons, protons, and neutrons found in an atom?

a)
Electrons are in the nucleus; protons and neutrons are in the electron cloud.
b)

Electrons are orbiting the nucleus; protons and neutrons are in the nucleus.

c)
All particles are found in the nucleus.
d)
Electrons are in the nucleus; protons are in the electron cloud.
61.

How do you calculate the atomic number of an atom?

a)
The atomic number is calculated by adding the number of neutrons and protons.
b)
The atomic number is equal to the number of protons in the atom.
c)
The atomic number is the total number of electrons in the atom.
d)
The atomic number is the mass of the atom divided by its volume.
62.

How do you calculate the charge of an atom?

a)
The charge of an atom is determined by its mass.
b)
The charge of an atom is equal to the number of neutrons.
c)
The charge of an atom is calculated by the difference between the number of protons and electrons.
d)
The charge of an atom is calculated by adding the number of protons and neutrons.
63.

How do you calculate the mass number of an atom?

a)
The mass number is the total number of chemical bonds in an atom.
b)
The mass number is the average atomic mass of all isotopes.
c)
The mass number is the sum of protons and neutrons in an atom.
d)
The mass number is the number of electrons in an atom.
64.

What are a positively and negatively charged atom called, respectively?

a)
Cation and Anion
b)
Electron and Positron
c)
Proton and Neutron
d)
Molecule and Ion
65.

What factor identifies the element: atomic number, mass number, or charge?

a)
atomic number
b)
charge
c)
mass number
d)

none

66.

Where are the mass number, charge, and atomic number written in isotopic notation?

a)
Mass number is written on the right, atomic number on the left, and charge is omitted.
b)

Mass number is top left, atomic number is bottom left, charge is top right.

c)
Mass number is subscript right, atomic number is superscript right, charge is superscript left.
d)
Mass number is subscript left, atomic number is superscript left, charge is subscript right.
67.

What are isotopes?

a)

Isotopes are atoms of the same element that have but different masses.

b)
Isotopes are elements with different numbers of protons.
c)
Isotopes are the same as ions but with different charges.
d)
Isotopes are elements that have the same atomic mass.
68.

What is mass spectroscopy?

a)
A technique for analyzing the color of substances.
b)
A method for measuring temperature changes in gases.
c)

Mass spectroscopy is an analytical technique for measuring the mass of ions.

d)
A process for determining the density of liquids.
69.

What is atomic mass?

a)
Atomic mass is the total number of protons in an atom.
b)
Atomic mass is the mass of an atom without considering isotopes.
c)
Atomic mass is the mass of an electron in an atom.
d)

Atomic mass is the weighted average mass of atoms; measured in amu

70.

What is the equation for average atomic mass?

a)

Average Atomic Mass = Σ (% of abundance x atomic mass) / 100

b)
Average Atomic Mass = (isotope mass - fractional abundance) / total isotopes
c)
Average Atomic Mass = (isotope mass + fractional abundance)
d)
Average Atomic Mass = (isotope mass × total isotopes)
71.

How do you calculate the mass of a molecule?

a)
The mass of a molecule is the same as its boiling point.
b)
The mass of a molecule is determined by its volume.
c)
The mass of a molecule is calculated by summing the atomic masses of all atoms in its molecular formula.
d)
The mass of a molecule is calculated by dividing its density by its volume.
72.

What is the only difference in the process of calculating atomic mass and molar mass of a molecule?

a)

The only difference is that atomic mass is measured in amu and molar mass is measured in g/mol.

b)
Atomic mass is based on the molecular structure, while molar mass is not.
c)
Molar mass is calculated using only the most abundant isotope of each element.
d)
Atomic mass is always a whole number, while molar mass is a decimal.
73.

What is the equation for molar mass, in terms of grams and moles?

a)
Molar Mass = Moles (mol) / Mass (g)
b)
Molar Mass = Mass (g) + Moles (mol)
c)
Molar Mass = Mass (g) * Moles (mol)
d)
Molar Mass = Mass (g) / Moles (mol)
74.

How des you calculate molarity/solution?

a)
Molarity (M) = grams of solute / liters of solution
b)
Molarity (M) = moles of solute x liters of solution
c)
Molarity (M) = liters of solution / moles of solute
d)
Molarity (M) = moles of solute / liters of solution
75.

What is the difference between saturated and unsaturated?

a)

Saturated compounds are homogenous while unsaturated compounds are heterogenous.

b)
Saturated compounds have more hydrogen atoms than unsaturated compounds.
c)
Unsaturated compounds are always solid at room temperature.
d)
Saturated compounds contain fewer carbon atoms than unsaturated compounds.
76.

When measuring, how many digits should be a guess?

a)
One additional digit beyond the precision of the measuring instrument.
b)
No additional digits are needed for guessing.
c)
The same number of digits as the measuring instrument.
d)
Two additional digits beyond the precision of the measuring instrument.
77.

Do opposite charges attract or repel?

a)

Attract

b)

Repel

c)

Both

d)

Neither

78.

What is the charge on a proton, alpha particle, and positron?

a)

Negative

b)

Positive

c)

Neutral

79.

What is the charge of a beta particle and an electron?

a)

Neutral

b)

Positive

c)

Negative

80.

What is the charge of a gamma particle?

a)

Positive

b)

Neutral

c)

Negative

81.

What happened in the gold foil experiment?

a)
The gold foil experiment indicated that all matter is made of gold.
b)
The gold foil experiment proved that atoms are indivisible.
c)
The gold foil experiment showed that electrons are located in the nucleus.
d)
The gold foil experiment demonstrated that atoms have a small, dense nucleus.
82.

What happened in the plum model?

a)
The plum model suggested that atoms are solid spheres without any internal structure.
b)
The plum model proposed that atoms consist of a positive matrix with embedded electrons.
c)
The plum model indicated that electrons orbit the nucleus like planets around the sun.
d)
The plum model claimed that atoms are made entirely of negatively charged particles.
83.

What was the cathode ray experiment?

a)
The cathode ray experiment demonstrated the existence of electrons as negatively charged particles.
b)
The cathode ray experiment showed that light is made of particles called photons.
c)
The cathode ray experiment was conducted to discover the neutron.
d)
The cathode ray experiment proved the existence of protons as positively charged particles.
84.

Who developed the current model of an atom?

a)

Bohr

b)

Newton

c)
Marie Curie
d)
Albert Einstein
85.

What is the equation for percentage of abundance/# of grams?

a)
(total grams - number of grams of substance) * 100
b)
(number of grams of substance + total grams) * 100
c)
(total grams / number of grams of substance) * 100
d)

(total grams / 100 mL) * 100

86.

What is molarity?

a)
Molarity is the volume of solute in milliliters per liter of solution.
b)
Molarity is the mass of solute per liter of solution.
c)

Molarity is the amount of substance in a given volume.

d)
Molarity is the number of moles of solvent per liter of solution.
87.

What is the correct order of these from longest to shortest wavelengths: gamma ray, infared, radio, microwave, visible?

a)
visible, gamma ray, microwave, infrared, radio
b)
radio, microwave, visible, gamma ray, infrared
c)
infrared, radio, gamma ray, visible, microwave
d)

radio, microwave, infared, visible, gamma ray

88.

What is electron configuration?

a)
The process of electron transfer between atoms.
b)

Electron configuration is the arrangement of electrons that defines the properties and functions of elements.

c)
The measurement of an atom's mass.
d)
The speed at which electrons move in a conductor.
89.

True or False: Elements in the same column of the periodic tables have similar chemical properties because they have similar electron configurations.

a)

True

b)

False

90.

What determines the column that an element is in?

a)

The number of valance electrons.

b)
The state of matter of the element.
c)
The color of the element.
d)
The mass of the element.
91.

What determines the period an element is in?

a)
The highest energy level of electrons (number of electron shells).
b)
The atomic number of the element.
c)
The number of protons in the nucleus.
d)
The element's reactivity with other substances.
92.

What is an orbital?

a)
An orbital is a type of particle found in the nucleus of an atom.
b)
An orbital is a region in an atom where there is a high probability of finding an electron.
c)
An orbital is a fixed path that electrons follow around the nucleus.
d)
An orbital is a measure of the energy level of an atom.
93.

What determines the size and shape of orbitals, respectively?

a)
The number of protons in the nucleus determines the size, and the principal quantum number (n) determines the shape of orbitals.
b)
The energy level of the atom determines the size, and the magnetic quantum number (m) determines the shape of orbitals.
c)

The number of energy levels determines the size and the sub-shells determines the shape.

d)
The mass of the electron determines the size, and the spin quantum number (s) determines the shape of orbitals.
94.

What are the 4 types of sub-shells?

a)
1, 2, 3, 4
b)
x, y, z, w
c)
s, p, d, f
d)
g, h, i, j
95.

What are the number of orbitals associated with each of the types of sub-shells?

a)
s: 2, p: 4, d: 6, f: 8
b)
s: 1, p: 2, d: 3, f: 4
c)
s: 1, p: 3, d: 4, f: 5
d)
s: 1, p: 3, d: 5, f: 7
96.

How do you draw orbitals in the orbital filling form?

a)

Write a line and then two arrows (going in opposite directions) representing electrons.

b)
Draw orbitals as random squiggles without any structure.
c)
Use only colors to represent orbitals without shapes.
d)
Draw orbitals as flat 2D shapes on paper.
97.

What does Inert mean?

a)
Inert means highly reactive.
b)
Inert refers to a state of being active.
c)
Inert is a term for explosive materials.
d)

Inert means not reactive or chemically inactive (when atoms have 8 electrons).

98.

What is noble gas electron configuration?

a)
It describes the arrangement of protons in an atom.
b)
It is a method to calculate atomic mass.
c)
It refers to the color of noble gases in the periodic table.
d)
The noble gas electron configuration is a shorthand notation that uses the electron configuration of the nearest noble gas to represent the electron arrangement of an element.
99.

What is the rule for special electron configurations in the d-subshell (d4 and d9)?

a)

Electrons in d4 and d9 configurations are promoted from the s-subshell to achieve half-filled (d5) or fully filled (d10) stability. To do this, you must take an electron from the previous electron value.

b)
Electrons in d4 and d9 configurations are added from the p-subshell instead of the s-subshell.
c)
Electrons in d4 and d9 configurations remain in the d-subshell without promotion.
d)
d4 and d9 configurations are always stable without any adjustments.
100.

What is the rule for excited state electron configuration? How can you spot them?

a)

Excited state electron configurations have electrons in higher energy levels than the ground state. Not all lower energy levels will be filled (ex: 3s2 4s1 to 3s1 4s2).

b)
Excited state configurations have all electrons in the lowest energy levels.
c)
Excited state configurations only occur in noble gases.
d)
Excited state configurations have fewer electrons than the ground state.
101.

What is photoelectron spectroscopy?

a)

Photoelectron spectroscopy is a technique for analyzing the electronic structure of materials by measuring the energy of ejected electrons (basically electron configuration on a graph).

b)
An analysis method for determining the mass of molecules.
c)
A technique for visualizing the surface of materials using light.
d)
A method for measuring temperature changes in materials.
102.

What are the three main rules for writing electron configuration?

a)

Aufbau Principle = electrons must first enter the lowest energy levels, Pauli Exclusion Principle = each orbital can have no more than 2 electrons in opposite spins, Hund's Rule = one electrons must occupy each orbital before doubling up.

b)
Thermodynamic Law
c)
Relativity Principle
d)
Quantum Theory
103.

What are the special rules when writing the electron configuration of d and f block elements?

a)
Remove electrons from 3d before 4s when forming anions.
b)
Always fill the 4p subshell before the 4s subshell.
c)

For d-block elements, subtract 1 from the energy level and for f-block elements subtract 2 from the energy level.

d)
Fill the 3d subshell before the 4s subshell; add electrons to 3d when forming cations.
104.

What is the process for writing a elements' standard form electron configuration?

a)
Electrons are placed in orbitals based solely on their spin direction.
b)
The standard form requires filling all orbitals before moving to the next energy level.
c)
The electron configuration is written by randomly assigning electrons to orbitals.
d)
The standard form electron configuration is written by filling orbitals in order of increasing energy, following the rules of the Aufbau principle, Hund's rule, and the Pauli exclusion principle.
105.

What is Na's electron configuration?

a)
1s² 2s² 2p⁶ 3p¹
b)
1s² 2s² 2p⁶ 3s²
c)
1s² 2s² 3s² 3p¹
d)
1s² 2s² 2p⁶ 3s¹
106.

How do you calculate the number of VEs and CEs based on electron configuration?

a)
Valence electrons are always equal to the number of protons.
b)
Core electrons are only found in the outermost shell.
c)
Valence electrons can be calculated by subtracting core electrons from total electrons.
d)

Valence electrons are the number of electrons in the highest energy level; core electrons are total electrons minus valence electrons.

107.

To reach 8 electrons, what do elements do?

a)
Elements can only lose electrons to reach 8.
b)
Elements only gain electrons to reach 8.
c)
Elements do not interact with electrons to reach 8.
d)

Elements gain, lose, or share electrons to reach 8 electrons (become the nearest noble gas).

108.

What is Electron Affinity?

a)
Electron affinity is the energy released when an atom loses an electron.
b)
Electron affinity measures the size of an atom.
c)
Electron affinity is the force that holds electrons in an atom.
d)

Electron affinity is the energy that it takes to add electrons one by one to an atom.

109.

What is the trend for electron affinity across a group and a period?

a)
Electron affinity increases down a group and decreases across a period.
b)
Electron affinity remains constant across a period and a group.
c)
Electron affinity decreases across a period and increases down a group.
d)
Electron affinity increases across a period and decreases down a group.
110.

What elements typically become cations? Which typically become anions?

a)
Metals become cations; nonmetals become anions.
b)
Metals become anions; nonmetals become cations.
c)
Noble gases become cations; alkali metals become anions.
d)
Transition metals become anions; alkaline earth metals become cations.
111.

What is the equation for effective nuclear charge?

a)
Z_eff = Z + S
b)
Z_eff = S - Z
c)
Z_eff = Z * S
d)

Z_eff = Z_protons - S_core

112.

What is the trend for electronegativity for a period and a group?

a)
Electronegativity decreases across a period and increases down a group.
b)
Electronegativity remains constant across a period and a group.
c)
Electronegativity increases down a group and decreases across a period.
d)
Electronegativity increases across a period and decreases down a group.
113.

What is an ionic bond?

a)

A type of bond that forms between a metal and a nonmetal (anion and cation).

b)
A weak attraction between neutral molecules.
c)
A type of bond that occurs only in metals.
d)
A bond formed by the sharing of electrons between atoms.
114.

What is a covalent bond?

a)

A covalent bond is a bond formed between two nonmetals.

b)
A covalent bond is formed by the attraction of oppositely charged ions.
c)
A covalent bond involves the transfer of electrons between atoms.
d)
A covalent bond is a type of ionic bond.
115.

What is a metallic bond?

a)

A metallic bond is a type of chemical bonds between two metals.

b)
A metallic bond is a strong bond formed by ionic interactions.
c)
A metallic bond involves the transfer of electrons from one atom to another.
d)
A metallic bond is a bond between non-metal atoms.
116.

Why do atoms react?

a)

Atoms react to achieve stability in their electron configurations. or to have 8 electrons.

b)
Atoms react to increase their mass.
c)
Atoms react to form larger molecules.
d)
Atoms react to emit light energy.
117.

What do you have to add to form the correct name of anions?

a)
Add '-ic' for simple anions
b)
Add 'ion' for polyatomic anions
c)
Add '-ous' for all anions
d)
Add '-ide' for simple anions and '-ate' or '-ite' for polyatomic anions.
118.

What needs to be done to properly name a compound?

a)
Count the number of atoms only
b)

Add a prefixes (mono,di,tri) and suffixes (ide, ate,ite)

c)
Ignore functional groups
d)
Use only common names
119.

What are the three ways in which valance electron participate in chemical reactions?

a)

Donating, Accepting, and Sharing

b)
Decomposition, condensation, and filtration.
c)
Ionization, crystallization, and evaporation.
d)
Catalysis, polymerization, and sublimation.
120.

What is the essential part of the Lewis dot structure?

a)
Molecular geometry depiction.
b)

Valence electrons representation as dots.

c)
Atomic number representation.
d)
Chemical bond strength indication.
121.

How is the type of ion formed by transition metals indicated?

a)
By the color of the metal in solution.
b)
By the size of the metal ions.
c)
By the position of the metal in the periodic table.
d)

By Roman numerals.

122.

What is the correct order of elements when writing an ionic compound?

a)
Anion first, then cation
b)
Cation and anion in any order
c)
Cation and anion must be combined together
d)
Cation first, then anion
123.

What is lattice energy?

a)
Lattice energy is the energy associated with the melting of ionic compounds.
b)

Lattice energy is the energy the holds the ions together in an ionic compound.

c)
Lattice energy is the energy absorbed when a solid ionic compound is formed from gaseous ions.
d)
Lattice energy is the energy required to break a solid ionic compound into gaseous ions.
124.

What is the trend for lattice energy in a group and a period?

a)
Lattice energy increases down a group and remains constant across a period.
b)

Lattice energy decreases down a group and increases across a period.

c)
Lattice energy decreases down a group and decreases across a period.
d)
Lattice energy remains constant down a group and increases across a period.
125.

What shift in charge and size increases lattice energy?

a)
Decrease in charge and decrease in size.
b)
Increase in charge and decrease in size.
c)
Increase in charge and increase in size.
d)
Decrease in charge and increase in size.
126.

Do ionic compounds conduct electricity when solid? Do they when liquified?

a)
Ionic compounds conduct electricity when solid and liquified.
b)
Ionic compounds conduct electricity only when solid.
c)
Ionic compounds do not conduct electricity when solid, but they do when liquified.
d)
Ionic compounds do not conduct electricity in any state.
127.

What are the two factors that lattice energy is affected by?

a)
Temperature of the ions
b)
Mass of the ions
c)
Electronegativity of the ions
d)
Charge of the ions and size of the ions
128.

What conducts electricity?

a)
Gases always conduct energy in solution.
b)
Non-ionic compounds in solution conduct energy.
c)

Ions (made when ionic compounds are dissolved).

d)

Metals in solid form.

129.

How do you calculate Lattice Energy?

a)

Lattice energy is calculated by adding up the absolute value of the charges in a compound.

b)
Lattice energy is found by averaging the atomic masses of the elements involved.
c)
Lattice energy can be determined by measuring the boiling point of a substance.
d)
Lattice energy is calculated using the ideal gas law.
130.

What is the difference between a polar and a nonpolar covalent bond?

a)
A polar covalent bond has equal sharing of electrons, while a nonpolar covalent bond has unequal sharing.
b)
Both polar and nonpolar covalent bonds involve equal sharing of electrons.
c)
A polar covalent bond has unequal sharing of electrons, while a nonpolar covalent bond has equal sharing.
d)
A polar covalent bond is formed between two metals, while a nonpolar covalent bond is formed between a metal and a nonmetal.
131.

What number must the subtracted electronegativities be for it to be a non-polar bond? A polar bond? An ionic bond?

a)

Polar bond: 0.0-0.4, Non polar bond: 0.5 to 1.7, Ionic bond: >1.7

b)

Non-polar bond: 0.0-0.3, Polar bond: 0.4 to 1.7, Ionic bond: >1.7

c)

Non-polar bond: 1.0 to 2.0, Polar bond: 2.0 to 3.5, Ionic bond: >3.5

d)
Ionic bond: <1.0
132.

What is the Lewis Structure?

a)
A representation of atomic mass in a compound.
b)
A method for calculating molecular weight.
c)

A diagram showing the arrangement of electrons and atoms in a molecule.

d)
A type of chemical reaction.
133.

What is formal charge?

a)
Formal charge is the actual charge of an atom in a molecule.
b)

Formal Charge = assigned VE - actual VE

c)

Formal Charge = actual VE - assigned VE

d)
Formal charge is the total number of protons in an atom.
134.

What are the 4 types of sharing electrons in the Lewis Structure?

a)
Single ionic bond
b)
Double ionic bond
c)

Single bond, Double bond, Triple bond, Quadrupal bond

d)

Loan Pairs, Single bond, Double bond, Triple bond

135.

What elements must have 8 VEs?

a)
Transition metals: iron, copper, nickel
b)
Halogens: fluorine, chlorine, bromine
c)

Period 2: C, N, O, F..

d)
Alkali metals: lithium, sodium, potassium
136.

What elements can only have a single bond?

a)
Nitrogen
b)
Oxygen
c)
Carbon
d)
Hydrogen and halogens (F, Cl, Br, I)
137.

What elements can have less than 8 VEs?

a)

Ar, K, and Cl

b)

H, Be, and B

c)
Elements in group 14 and 15
d)
Only alkali metals and alkaline earth metals
138.

What elements can have more than 8 VEs?

a)
Bromine, iodine, and chlorine
b)
Helium, neon, and argon
c)

Elements in period 1 or period 2

d)

Elements in period 3 and beyond

139.

What is resonance structure?

a)
Resonance structures are only applicable to ionic compounds.
b)
Resonance structures involve changing the atomic nuclei positions.
c)
Resonance structures are the same as the original Lewis structure.
d)
Resonance structures are alternative Lewis structures for a molecule that differ only in the placement of electrons.
140.

What is an Electron Domain?

a)
An electron domain is a region around a central atom where electrons are likely to be found.
b)
A type of chemical bond formed between atoms.
c)
A measure of the atom's mass.
d)
A region where protons are concentrated.
141.

What are Ion-Dipole forces?

a)
Interactions between two non-polar molecules.
b)
Forces that occur only in gases.
c)
Attractive forces between two ions of opposite charge.
d)
Ion-dipole forces are interactions between an ion and a polar molecule.
142.

What are Hydrogen bonds?

a)
Hydrogen bonds are formed only between hydrogen and oxygen atoms.
b)

Hydrogen bonds are bonds between a hydrogen atoms (N-H, O-H, or F-H) and an N, O, or F.

c)
Hydrogen bonds are strong covalent bonds between hydrogen atoms.
d)
Hydrogen bonds are permanent connections that do not break easily.
143.

What are Dipole-dipole forces?

a)
Dipole-dipole forces occur only in ionic compounds.
b)
Dipole-dipole forces are weak interactions between neutral atoms.
c)

Dipole-dipole forces are bonds between two polar molecules that is not a hydrogen bond.

d)
Dipole-dipole forces are repulsive forces between two nonpolar molecules.
144.

What are London-Dispersion forces?

a)
London-Dispersion forces are strong covalent bonds between atoms.
b)

London-Dispersion forces are weak intermolecular forces caused by temporary dipoles in molecules; the larger the molecules, the stronger the bond

c)
London-Dispersion forces are permanent dipoles in polar molecules.
d)
London-Dispersion forces are the result of ionic interactions between charged particles.
145.

What are Dipole-induced dipole bonds?

a)
Covalent bonds formed between polar and nonpolar molecules
b)
Repulsive forces between two nonpolar molecules
c)
Attractive forces between two polar molecules
d)

Dipole-induced dipole bonds are attractive forces between a polar molecule and a nonpolar molecule.

146.

What is stoichiometry?

a)
Stoichiometry refers to the measurement of temperature changes in reactions.
b)
Stoichiometry is the study of animal behavior.
c)
Stoichiometry is the calculation of reactants and products in chemical reactions.
d)
Stoichiometry is the analysis of sound waves in chemistry.
147.

True or False: the ratio established in a chemical equation can be used to do calculations when given a certain amount of one of the molecules in the reaction?

a)

True

b)

False

c)

Both

148.

What is the limiting reagent?

a)
The limiting reagent is the product formed in the reaction.
b)
The limiting reagent is the reactant that is in excess.
c)

The limiting reagent is the reactant that is used up in a chemical reaction. It produces less product than the excess reagent.

d)
The limiting reagent is the catalyst used in the reaction.
149.

What is the Excess Reagent?

a)
The excess reagent is the reactant that is completely consumed in a chemical reaction.
b)
The excess reagent is the product formed in a chemical reaction.
c)
The excess reagent is the catalyst that speeds up the reaction.
d)

The excess reagent is the reactant that is not completely used up in a chemical reaction. It produces more product than the limiting reagent.

150.

What are the 4 steps to finding the limiting reagent and the max amount of product that is able to be made?

a)
1) Write the balanced equation, 2) Identify the products, 3) Calculate total moles, 4) Determine limiting reagent.
b)

The 4 steps are: 1) Write the balanced equation, 2) Convert to moles, 3) Identify the limiting reagent, (by calculating max product for both), 4) Calculate maximum product (process of elimination).

c)
1) Write the balanced equation, 2) Convert to liters, 3) Identify the reactants, 4) Calculate theoretical yield.
d)
1) Write the unbalanced equation, 2) Convert to grams, 3) Calculate the excess reagent, 4) Estimate product yield.
151.

What are the 4 things that need to be multiplied to find total product given a set amount of reactant (in grams)?

a)

[Amount of reactant (g) / 1] x [1 / Molar mass(R)] x Conversion factor x [Molar Mass(P) / 1]

b)
Amount of reactant (g) x Stoichiometric ratio x Energy input x Catalyst amount
c)
Amount of product (g) x Molar mass (g/mol) x Reaction time x Yield
d)
Amount of reactant (g) x Molar volume (L/mol) x Temperature x Pressure
152.

What is reaction kinetics?

a)
The study of chemical compounds
b)
The analysis of molecular structures
c)
The examination of physical properties of substances
d)
Reaction kinetics is the branch of chemistry that deals with the rates of chemical reactions.
153.

What 2 things are needed for proper collisions in chemical reactions?

a)
Random mixing of reactants
b)
High temperature and low pressure
c)
Sufficient energy and correct orientation
d)
Presence of a catalyst only
154.

What 4 things affect the rate of a reaction the most?

a)
Temperature, concentration, surface area, and catalysts
b)
Pressure, humidity, volume, and light
c)
pH, magnetic fields, time, and distance
d)
Solubility, viscosity, density, and color
155.

How does temperature impact the rate of a reaction?

a)
Temperature has no effect on reaction rates.
b)

Temperature increases the rate of a reaction by increasing the kinetic energy of reactants.

c)
Higher temperatures slow down molecular collisions.
d)
Temperature only affects solid-state reactions.
156.

How does surface area impact the rate of a reaction?

a)
Surface area only affects solid reactants, not liquids or gases.
b)

Surface area increases the rate of a reaction by allowing proper orientation areas for collisions to occurs.

c)
Increasing surface area decreases the rate of a reaction.
d)
Surface area has no effect on reaction rates.
157.

How do catalysts impact the rate of a reaction?

a)
Catalysts increase the rate of a reaction by lowering the activation energy.
b)
Catalysts only work at high temperatures to speed up reactions.
c)
Catalysts have no effect on the rate of a reaction.
d)
Catalysts decrease the rate of a reaction by increasing the activation energy.
158.

How does concentration impact the rate of a reaction?

a)

Higher concentration increases the amount of molecules and thus increases the chance of collisions which increases the rate of a reaction.

b)
Lower concentration increases the rate of reaction.
c)
Concentration has no effect on the rate of reaction.
d)
Higher concentration decreases the rate of reaction.
159.

What happens to the concentration of reactants during a reaction? What about the concentration of products?

a)
The concentration of reactants increases, while products remain unchanged.
b)
The concentration of reactants remains constant, while products decrease.
c)
Both reactants and products increase in concentration during the reaction.
d)
The concentration of reactants decreases, while the concentration of products increases.
160.

What do coefficients tell about the rate of a reaction?

a)
Coefficients represent the temperature of the reaction.
b)

Coefficients show the relative amounts of reactants and products; a higher coefficient means a reactant is being used faster and vice versa.

c)
Coefficients determine the color change during the reaction.
d)
Coefficients indicate the pressure required for the reaction.
161.

What does it mean for a chemical reaction to be in equilibrium?

a)
The concentration of reactants is always greater than products at equilibrium.
b)
Equilibrium means the reaction only proceeds in one direction.
c)
A chemical reaction is in equilibrium when the rates of the forward and reverse reactions are equal.
d)
The reaction stops completely when in equilibrium.
162.

What are the comparative energy levels of products and reactants in an endothermic reaction? In an exothermic reaction?

a)
Endothermic: products = reactants; Exothermic: products < reactants
b)
Endothermic: products < reactants; Exothermic: products > reactants
c)
Endothermic: products > reactants; Exothermic: products < reactants
d)
Endothermic: products < reactants; Exothermic: products = reactants
163.

What is the peak of the curve on a chemical reaction graph called?

a)

Activated complex

b)

Transition State

c)
Energy barrier height
d)
Catalyst threshold
164.

What is Ea?

a)
Reaction rate constant
b)
Thermodynamic potential
c)

Activation energy

d)
Energy barrier
165.

What are ΔH and ΔG in a chemical reaction graph?

a)
ΔH is the change in mass; ΔG is the change in concentration.
b)

ΔH is the change in enthalpy; ΔG is the change in Gibbs free energy; both are energy in a reaction (H on top, G on the bottom).

c)
ΔH is the change in temperature; ΔG is the change in entropy.
d)
ΔH is the change in pressure; ΔG is the change in volume.
166.

On a pH scale, what are things below 7 called? What are things above 7 called?

a)
Neutral for pH below 7; Acidic for pH above 7.
b)
Basic for pH below 7; Neutral for pH above 7.
c)
Alkaline for pH below 7; Acidic for pH above 7.
d)
Acidic for pH below 7; Basic (or Alkaline) for pH above 7.
167.

What is an acid?

a)
An acid is a base in chemical reactions.
b)
An acid is a proton acceptor in chemical reactions.
c)
An acid is a type of salt in chemistry.
d)

An acid is a H+ donor or producer.

168.

What is a Base?

a)
A base is a type of acid that donates protons.
b)
A base is a substance that only accepts electrons.
c)
A base is a solution that has a pH below 7.
d)

A base is a substance that donates OH- or the can accept H+.

169.

What is the tell tale sign that something is an acid? What is the sign that is a base?

a)
Acids have a bitter taste; bases are sour.
b)
Acids turn red litmus paper blue; bases turn blue litmus paper red.
c)

Acids have an H in front; Bases have a 1st or 2nd group element + OH or have N.

d)

Bases have an H in front; Acids have a 1st or 2nd group element + OH or have N.

170.

What must most chemical reactions have (in terms of acids and bases)?

a)
The formation of a gas without any acid or base involvement.
b)

An acid and a base.

c)
A change in temperature without any chemical change.
d)
A reaction that only involves electrons transfer.

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