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Honors Chemistry Review

Total questions: 115

Worksheet time: 2hrs 55mins

Name
Class
Date
1.

What is the name of group one on the periodic table?

a)

Alikali metals

b)

Alkaline earth metals

c)

halogens(salt former)

d)

noble gasses

e)

transition metals

2.

what is the name of group 2 on the periodic table?

a)

alikali metals

b)

alkaline earth metals

c)

transition metals

d)

halogens(salt former)

e)

noble gasses

3.

what is the name for groups 3-12 on the periodic table?

a)

Alikali metals

b)

alkaline earth metals

c)

transition metals

d)

noble gasses

e)

halogens(salt former)

4.

what is the name for groups 17 on the periodic table?

a)

Alkali metals

b)

Alkaline earth metals

c)

transition metals

d)

Halogens(salt former)

e)

noble gasses

5.

What is the name for groups 18 on the periodic table?

a)

Alkali metals

b)

Alkaline earth metals

c)

transition metals

d)

Halogens(salt former)

e)

Noble gasses

6.

What is the name for La-Lu

a)

Halogens(salt former)

b)

Actanides

c)

Lanthanides

d)

Alkaline earth metals

e)

noble gasses

7.

What is the name of Ac-Lr

a)

lanthanides

b)

Actanides

c)

noble gasses

d)

Alikali metals

e)

transition metals

8.

how many valence electrons does group 1(Alikali metals) have?

(a)  

9.

How many valence electrons does group 2(Alkaline earth metals) have?

(a)  

10.

What is the name of group 13?

a)

Boron group

b)

Carbon group

c)

Nitrogen group

d)

Oxygen group

11.

what is the name of group 14?

a)

Boron group

b)

carbon group

c)

nitrogen group

d)

oxygen group

12.

What is the name for group 15?

a)

Boron group

b)

carbon group

c)

nitrogen group

d)

oxygen group

13.

whats the name for groups 16?

a)

Boron group

b)

carbon group

c)

nitrogen group

d)

oxygen group

14.

Boron group has (a)   valence electrons

15.

The carbon group has (a)   valence electrons

16.

The nitrogen group has (a)   valence electrons

17.

the oxygen group has (a)   valence electrons

18.

the Halogens have (a)   valence electrons

19.

The noble gasses have (a)   valence electrons

20.

which elements want to gain electrons

a)

Nonmetals

b)

Metals

21.

which elements want to lose electrons

a)

Metals

b)

nonmetals

22.

Charge of group 1?

(a)  

23.

Charge of group 2?

(a)  

24.

Charge of group 13?

(a)  

25.

Charge of group 14?

(a)  

26.

Charge of group 15?

(a)  

27.

Charge of group 16?

(a)  

28.

Charge of group 17?

(a)  

29.

Charge of group 18?

(a)  

30.

Which elements have more than one charge or positive oxidation number?

a)

alkaline earth metals

b)

halogens

c)

Transition metals

d)

noble gasses

31.

Where are the metals located on the periodic table?

a)
Left side of the periodic table
b)
Right side of the periodic table
c)
In the middle of the periodic table
d)
At the top of the periodic table
32.

where are the metalloids located on the periodic table?

a)
In the alkali metals section
b)
Along the staircase line
c)
In the lanthanides and actinides section
d)
In the noble gases section
33.

Where are the nonmetals located on the periodic table?

a)
On the left side of the periodic table
b)
In the middle of the periodic table
c)
At the top of the periodic table
d)
On the right side of the periodic table
34.

What are properties of metals?

a)
Dull, brittle, poor conductors of heat and electricity, low melting and boiling points
b)
Transparent, flexible, insulators of heat and electricity, low melting and boiling points
c)
Soft, non-reactive, liquid at room temperature, low density
d)
Shiny, malleable, ductile, good conductors of heat and electricity, high melting and boiling points
35.

What are properties of nonmetals?

a)
Poor conductors of heat and electricity, tend to gain electrons, brittle in solid form
b)
Highly reactive with water, conductive in all forms, ductile in solid form
c)
Good conductors of heat and electricity, tend to lose electrons, malleable in solid form
d)
Low melting point, high density, shiny appearance
36.

what are properties of metalloids?

a)
Semiconductors, intermediate properties between metals and nonmetals, varying physical properties, can conduct electricity under certain conditions
b)
Non-reactive, low thermal conductivity, magnetic
c)
Low density, poor conductors of electricity, brittle
d)
High melting points, good conductors of electricity, ductile
37.

Who discovered the electron?

a)
J.J. Thomson
b)
Isaac Newton
c)
Albert Einstein
d)
Marie Curie
38.

Who discovered the proton & nucleus with the gold foil experiment?

a)
Ernest Rutherford
b)
Isaac Newton
c)
Marie Curie
d)
Albert Einstein
39.

What does the law of conservation of mass say?

a)
Mass can be converted into energy
b)
Mass cannot be created or destroyed, only rearranged.
c)
Mass can be destroyed completely
d)
Mass can be created out of nothing
40.

What's the difference between an element, compound, and a mixture?

a)
An element consists of two or more types of atoms, a compound consists of only one type of atom, and a mixture is a combination of substances that are chemically bonded.
b)
An element consists of two or more different types of atoms chemically bonded, a compound consists of only one type of atom, and a mixture is a combination of substances that are not chemically bonded.
c)
An element consists of two or more different types of atoms chemically bonded, a compound consists of two or more different types of atoms chemically bonded, and a mixture is a combination of substances that are not chemically bonded.
d)
An element consists of only one type of atom, a compound consists of two or more different types of atoms chemically bonded, and a mixture is a combination of substances that are not chemically bonded.
41.

Which color of visible spectrum has the longest wavelength and least energy?

a)
red
b)
green
c)
blue
d)
yellow
42.

Which color of visible spectrum is the most energetic?

a)
Red
b)
Violet
c)
Green
d)
Yellow
43.

When do we see light of a certain color given off by an element ?

a)
When the element is in a solid state
b)
When the electrons of an element fall back to their original energy levels after being excited.
c)
When the element is exposed to extreme heat
d)
When the element is mixed with water
44.

Formula for calculation wavelength?

a)
Wavelength = Frequency / Speed of Light
b)
Wavelength = Frequency * Speed of Light
c)
Wavelength = Speed of Light - Frequency
d)
Wavelength = Speed of Light / Frequency
45.

formula for calculating frequency?

a)
frequency = c - λ
b)
frequency = c + λ
c)
frequency = c * λ
d)
frequency = c / λ
46.

what kind of elements come together for covalent bonds?

a)
Metallic elements
b)
Noble gases
c)
Alkali metals
d)
Non-metallic elements
47.

What do the non-metallic elements do with their electrons when they come together for covalent bonds?

a)
They donate electrons.
b)
They absorb electrons.
c)
They release electrons.
d)
They share electrons.
48.

what kind of elements come together for ionic bonds?

a)
Metal and metal elements
b)
Nonmetal and metal elements
c)
Metal and nonmetal elements
d)
Metalloid and nonmetal elements
49.

What do the elements of ionic bonds do with their electrons when they come together for ionic bonds?

a)
Share electrons
b)
Absorb electrons
c)
Ignore electrons
d)
Transfer electrons
50.

What Is a formula unit?

a)
The number of atoms in a compound
b)
The molecular weight of a compound
c)
The charge of an ion in a compound
d)
The simplest ratio of elements in a compound
51.

HOw many ions are in one formula unit of MgCl2?

a)
3
b)
1
c)
4
d)
5
52.

What is an electrolyte?

a)
An electrolyte is a substance that does not conduct electricity in water.
b)
An electrolyte is a substance that enhances dehydration.
c)
An electrolyte is a substance that conducts electricity when dissolved in water or melted.
d)
An electrolyte is a substance that is only found in solid form.
53.

What is a nonelectrolyte?

a)
A nonelectrolyte is a substance that conducts electricity when dissolved in water.
b)
A nonelectrolyte is a substance that dissociates into ions when dissolved in water.
c)
A nonelectrolyte is a substance that increases conductivity in water.
d)
A nonelectrolyte is a substance that does not dissociate into ions when dissolved in water.
54.

What are two types of covalent bonds?

a)
Polar covalent bonds and nonpolar covalent bonds
b)
Hydrogen covalent bonds
c)
Metallic covalent bonds
d)
Ionic covalent bonds
55.

Why are metals malleable, ductile, and conductive?

a)
Metals are malleable, ductile, and conductive due to their high acidity
b)
Metals are malleable, ductile, and conductive due to their lack of atomic structure
c)
Metals are malleable, ductile, and conductive due to their atomic structure and the presence of free electrons.
d)
Metals are malleable, ductile, and conductive due to their non-metallic properties
56.

What particles are in the nucleus?

a)
Protons and neutrons
b)
Neutrons and electrons
c)
Electrons and protons
d)
Protons and positrons
57.

WHat is the charge of a proton?

a)
Positive
b)
Neutral
c)
Negative
d)
Zero
58.

What is the charge of an electron?

a)

-1.6 x 10^-20

b)

-1.6 x 10^-19

c)

-1.6 x 10^-18

d)

-1.6 x 10^-17

59.

what is the charge of a neutron?

a)
Half
b)
Negative
c)
Neutral
d)
Positive
60.

Which particles inside a neutral atom have to be equal?

a)
electrons and positrons
b)
neutrons and electrons
c)
protons and neutrons
d)
protons and electrons
61.

How do you write a nuclear symbol for an element?

a)
ElementSymbol^MassNumber-atomicNumber
b)
ElementSymbol^MassNumber_atomicNumber
62.

How do you write an electron configuration for an element?

a)
Write the electron configuration in alphabetical order of the elements
b)
Use the atomic number to determine the electron configuration
c)
Assign electrons randomly to energy levels and sublevels
d)
Follow the Aufbau principle and list the number of electrons in each energy level and sublevel.
63.

How do you write a noble gas configuration?

a)
Noble gas configuration is only used for metals
b)
Noble gas configuration is not relevant in chemistry
c)
The noble gas configuration for chlorine is [He] 3s2 3p5
d)
For example, the noble gas configuration for chlorine (Cl) is [Ne] 3s2 3p5, where [Ne] represents the electron configuration of neon.
64.

Write the electron configuration for Br

a)
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6
b)
1s2 2s2 2p6 3s2 3p6 4s2 3d9 4p6
c)
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5
d)
1s2 2s2 2p6 3s2 3p6 4s2 3d8 4p6
65.

Write the noble gas configuration for Se

a)
Xe 3d10 4s2 4p4
b)
Ne 3d10 4s2 4p4
c)
Kr 3d10 4s2 4p4
d)
[Ar] 3d10 4s2 4p4
66.

Tell me the period, group, block, and type of element for [Ar]4s2 3d10 4p3?

a)
Period: 3, Group: 12, Block: s, Type: Metal
b)
Period: 5, Group: 17, Block: d, Type: Metalloid
c)
Period: 4, Group: 15, Block: p, Type: Nonmetal
d)
Period: 6, Group: 14, Block: f, Type: Noble Gas
67.

How many electrons and the S sublevel hold?

a)
4
b)
6
c)
2
d)
8
68.

How many electrons can the P sublevel hold?

a)
10
b)
8
c)
6
d)
2
69.

How many electrons can the D sublevel hold?

a)
10
b)
8
c)
12
d)
5
70.

How many sublevels can the f sublevel hold?

a)
7
b)
12
c)
9
d)
4
71.

How do you calculate an electronegativity difference?

a)
Electronegativity difference = Electronegativity of less electronegative element - Electronegativity of more electronegative element
b)
Electronegativity difference = Electronegativity of more electronegative element - Electronegativity of less electronegative element
c)
Electronegativity difference = Electronegativity of more electronegative element + Electronegativity of less electronegative element
d)
Electronegativity difference = Electronegativity of more electronegative element / Electronegativity of less electronegative element
72.

What electronegativity difference EN will give a nonpolar covalent bond?

a)
0.5
b)
0.8
c)
0.3
d)
1.2
73.

What electronegativity difference EN will give a polar covalent bond?

a)
0.5 to 1.7
b)
2.0 to 3.0
c)
1.7 to 2.5
d)
0.2 to 0.8
74.

What electronegativity difference EN will give an ionic bond?

a)

EN less than 1.7

b)

EN equal to 1.7

c)

EN less than 2.0

d)

EN greater than 1.7

75.

Calculate the electronegativity for the bond between N-O and identify the bond type

a)
Ionic bond
b)
Polar covalent bond
c)
Nonpolar covalent bond
d)
Metallic bond
76.

Draw SO2, determine its ABE, geometry, polarity, and what intermolecular forces are involved

a)

a trigonal planar geometry, is a nonpolar molecule, and exhibits hydrogen bonding as intermolecular forces.

b)

a bent geometry, is a polar molecule, and exhibits dipole-dipole interactions and London dispersion forces as intermolecular forces.

c)

tetrahedral geometry, is a polar molecule, and exhibits metallic bonding as intermolecular forces.

d)

a linear geometry, is a nonpolar molecule, and exhibits ionic bonds as intermolecular forces.

77.

what is a period and how many are there(Chemistry)?

a)

horizontally-7

b)

vertically-5

c)

horizontally-9

d)

vertically-11

78.

What's a group and how many are there?

a)

vertically-18

b)

horizontally-36

c)

vertically-24

d)

horizontally-12

79.

write the number 0.0000576 into scientific notation with correct sig figs

a)
5.76 x 10^-5
b)
5.76 x 10^-6
c)
5.67 x 10^-5
d)
5.76 x 10^5
80.

What is the formula for density?

a)
Density = Volume / Mass
b)
Density = Mass x Volume
c)
Density = Mass / Volume
d)
Density = Weight / Volume
81.

what are the units used for density?

a)
liters per square meter (L/m^2)
b)
meters per second (m/s)
c)
grams per cubic centimeter (g/cm^3) or kilograms per cubic meter (kg/m^3)
d)
pounds per gallon (lb/gal)
82.

What is the density of water?

a)
2 g/cm^3
b)
0.5 g/cm^3
c)
3 g/cm^3
d)
1 g/cm^3
83.

what does the periodic law state?

a)
The properties of elements are periodic functions of their atomic numbers.
b)
The properties of elements are constant functions of their atomic masses.
c)
The properties of elements are linear functions of their atomic weights.
d)
The properties of elements are random functions of their atomic numbers.
84.

Who developed the first periodic table?

a)
Isaac Newton
b)
Dmitri Mendeleev
c)
Albert Einstein
d)
Marie Curie
85.

where are valence electrons?

a)
Valence electrons are located in the nucleus of an atom.
b)
Valence electrons are evenly distributed throughout all shells of an atom.
c)
Valence electrons are found in the innermost shell of an atom.
d)
Valence electrons are located in the outermost shell of an atom.
86.

what are valence electrons?

a)
Valence electrons are the electrons in the innermost shell of an atom
b)
Valence electrons are the electrons in the nucleus of an atom
c)
Valence electrons are the electrons in the outermost shell of an atom that are involved in chemical bonding.
d)
Valence electrons are the electrons that are not involved in chemical bonding
87.

what is an octet?

a)
An octet in chemistry refers to having a full outer shell of electrons, typically eight electrons.
b)
An octet in chemistry refers to a unit of measurement for atomic mass
c)
An octet in chemistry refers to a type of chemical reaction involving eight molecules
d)
An octet in chemistry refers to a group of eight elements in the periodic table
88.

If elements are similar they are in the same____?

a)
group
b)

period

89.

WHich elements can multiple bond?

a)
Hydrogen
b)

Halogens

c)
Phosphorus
d)

CONS

90.

Which type of compound is strong, high melting point, and conducts electricity when dissolved(electrolyte)?

a)
Organic compound
b)
Metallic compound
c)
Ionic compound
d)
Covalent compound
91.

which type of compound is weak, low melting point, and does not conduct electricity?

a)
Ionic compound
b)
Metallic compound
c)
Hydrogen compound
d)
Covalent compound
92.

what are the types of intermolecular forces?

a)

London dispersion forces, dipole-dipole, and hydrogen bonding

b)
Van der Waals forces, ionic bonding, metallic bonding
c)
Ionic bonding, covalent bonding, metallic bonding
d)
Hydrophobic interactions, ionic bonding, covalent bonding
93.

Which intermolecular forces are found in all covalent substances?

a)
Dipole-dipole interactions
b)
London dispersion forces
c)
Hydrogen bonding
d)
Ionic bonds
94.

Which intermolecular forces are found in polar covalent substances?

a)
Dipole-dipole interactions and London dispersion forces
b)
Ionic bonds and hydrogen bonding
c)
Van der Waals forces and metallic bonding
d)
Hydrogen bonding and covalent bonds
95.

Why is water so strong?

a)
Hydrogen bonding
b)

dipole dipole

c)
Covalent bonding
d)
Ionic bonding
96.

What are some unique properties of water

a)
Low surface tension, low specific heat capacity
b)
High surface tension, high specific heat capacity, universal solvent properties, maximum density at 4 degrees Celsius
97.

What is exothermic?

a)
Exothermic refers to a process that absorbs energy in the form of heat.
b)
Exothermic is a term used for reactions that occur at low temperatures.
c)
Exothermic describes a reaction that does not involve any energy change.
d)
Exothermic refers to a process or reaction that releases energy in the form of heat.
98.

WHat is endothermic?

a)
A process or reaction that absorbs heat from its surroundings.
b)
A process that releases heat to its surroundings
c)
A process that remains at a constant temperature
d)
A process that involves a phase change
99.

What is an isotope?

a)
Atoms of the same element with different numbers of neutrons.
b)
Compounds with varying atomic numbers
c)
Molecules of different elements
d)
Atoms with different numbers of electrons
100.

WHat is the most common state of matter in the universe, but not on earth?

a)
Gas
b)
Solid
c)
Plasma
d)
Liquid
101.

What are the states of matter?

a)
solid, liquid, gas, energy
b)
solid, liquid, gas, matter
c)
solid, liquid, gas, plasma
d)
solid, liquid, gas, air
102.

Which state of matter has the lowest density?

a)
Solid
b)
Plasma
c)
Gas
d)
Liquid
103.

Which state of matter has the highest density?

a)
Liquid
b)
Plasma
c)
Solid
d)
Gas
104.

Report 5.43x2.7 with correct sig figs

a)
13
b)
15
c)
14
d)
16
105.

give an example of an element

a)
Hydrogen (H)
b)
Gold (Au)
c)
Oxygen (O)
d)
Carbon (C)
106.

Example of a compound

a)
Oxygen (O)
b)
Nitrogen (N)
c)
Hydrogen (H)
d)
Water (H2O) and carbon dioxide (CO2) are examples of compounds.
107.

example of mixture

a)
Sugarwater
b)
Concrete
c)
Saltwater, air, soil
d)
Wood
108.

Use factor label method to convert 57.9km to mm

a)
579,000 mm
b)
5,790,000 mm
c)
579 mm
d)
57,900,000 mm
109.

convert 57.4 Ni to moles using factor label method

a)
0.456
b)
1.234
c)
0.978
d)
2.345
110.

what is the molar mass of CuCl2

a)
65.38 g/mol
b)
98.96 g/mol
c)
112.44 g/mol
d)
134.45 g/mol
111.

calculate the mass percent of each element in MgSO3

a)
{'Mg': 45.63%, 'S': 36.30%, 'O': 18.07%}
b)
{'Mg': 20%, 'S': 50%, 'O': 30%}
c)
{'Mg': 50%, 'S': 30%, 'O': 20%}
d)
{'Mg': 30%, 'S': 40%, 'O': 30%}
112.

how many sig figs are in 3500

a)
3
b)
4
c)
5
d)
2
113.

Scientific notation of 3500

a)
3.5 x 10^3
b)
350 x 10^1
c)
35 x 10^2
d)
3.5 x 10^2
114.

how many sig figs does 0.007890 have

a)
6
b)

7

c)
4
d)
3
115.

put 0.007890 into scientific notation

a)
78.90 x 10^-4
b)
7.890 x 10^-3
c)
7.89 x 10^-3
d)
0.789 x 10^-2

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