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Worksheetsfinal
Total questions: 120
Worksheet time: 4hrs 0mins
define chemistry
the science that seeks to understand what matter does by studying what atoms do
Anything that occupies space and has mass
the fundamental building blocks of matter
Types of atoms
define matter
anything that occupies space and has mass
The science that seeks to understand what matter does by studying what atoms do
the fundamental building blocks of matter
Types of atoms
True or False: The behavior of atoms determines the behavior of matter
true
false
define atoms
the fundamental building blocks of matter
Types of atoms
Anything that occupies space and has mass
Abbreviations for an elements
each___is a different type of atom
element
matter
chemistry
proton
True or False: Each element has unique properties that make it different from other elements
true
false
what are compounds
two or more elements joined together by chemical bonds
Indicates which atoms are present in a compound, and in what amount
Abbreviations for an elements
type of atom
The properties of compounds are the same as the properties of their constituent elements.
true
false
solids
Fixed shape and volume
Fixed volume, but no fixed shape
No fixed shape or volume
liquid
No fixed shape or volume
Fixed volume, but no fixed shape
fixed shape and volume
gases
No fixed shape or volume
Fixed volume, but no fixed shape
Fixed shape and volume
element
Made up of only one type of atom
Two or more elements joined together by chemical bonds
compound
Two or more elements joined together by chemical bonds
Made up of only one type of atom
pure substance
Composed of only one type of atom or compound
Composed of more than one type of atom or compound
mixture
Composed of more than one type of atom or compound
Composed of only one type of atom or compound
homogenous mixture
Composition is even throughout
Composition varies from one region to another
heterogenous mixture
Composition varies from one region to another
Composition is even throughout
aqueous solution
A homogeneous mixture of a substance dissolved in water
Matter that is composed of only one type of atom or molecule
A pure substance that is composed of only one type of atom
Pure substance in the liquid state
liquid
Pure substance in the liquid state
A mixture of water and another substance
A mixture with an even composition throughout
– A pure substance that is composed of two or more types of atoms
observation
Measurements or descriptions of the physical world
Explanations/ interpretations of observations that can be tested by further experimentation
Procedures designed to test hypotheses, theories, and scientific laws
Scientific laws summarize past observations and predict future events
hypothesis
Explanations or interpretations of observations that can be tested by further experimentation
Procedures designed to test hypotheses, theories, and scientific laws
Scientific laws summarize past observations and predict future events
Models that provide a broader and deeper explanation of observations and laws
experiment
Models that provide a broader and deeper explanation of observations and laws
Procedures designed to test hypotheses, theories, and scientific laws
Explanations or interpretations of observations that can be tested by further experimentation
Measurements or descriptions of the physical world
scientific laws
summarize past observations and predict future events
Models that provide a broader and deeper explanation of observations and laws
Procedures designed to test hypotheses, theories, and scientific laws
Explanations or interpretations of observations that can be tested by further experimentation
theories
Models that provide a broader and deeper explanation of observations and laws
Scientific laws summarize past observations and predict future events
Procedures designed to test hypotheses, theories, and scientific laws
Explanations or interpretations of observations that can be tested by further experimentation
True or False: Every part of the scientific method is subject to experimentation and revision
true
false
True or False: All numbers, including those in calculations, must include units
true
false
True or False: Intermediate values are rounded to the correct number of significant figures after every step in a multi-step calculation
true
false
density
The density of a substance is the ratio of its mass to its volume
Refinement or specificity of a measurement
The process of converting from one unit to another
Two quantities with different units known to represent the same amount
True or False: Atoms are mostly empty space
true
false
Which subatomic particle is the smallest
electron
neutron
proton
nucleus
where is most of an atoms mass located
outside nucleus
the nucleus
The identity of an element is determined by the number of __ in its ___
proton
neutron
electron
nucleus
What letter is used as an abbreviation for atomic number?
Z
A
M
E
what are isotopes
Atoms with the same number of protons, but different numbers of neutrons
Atoms with the same number of neutrons, but different numbers of proton
Atoms with the same number of protons and neutrons
mass number
The total number of protons and neutrons in an atom’s nucleus
The total number of neutrons in an atom’s nucleus
The total number of protons in an atom’s nucleus
What letter is used as an abbreviation for mass number?
Z
A
E
M
metals
Shiny when freshly cut ● Good conductors of heat and electricity ● Tend to bend rather than shatter when struck
Poor conductors of heat and electricity ● Tend to be either brittle solids or gases
Intermediate properties between metals and nonmetals ● Silicon - shiny like a metal, but brittle like a nonmetal.
non metals
Intermediate properties between metals and nonmetals ● Silicon - shiny like a metal, but brittle like a nonmetal.Poor conductors of heat and electricity ● Tend to be either brittle solids or gases
Poor conductors of heat and electricity ● Tend to be either brittle solids or gases
Shiny when freshly cut ● Good conductors of heat and electricity ● Tend to bend rather than shatter when struck
metalloids
Shiny when freshly cut ● Good conductors of heat and electricity ● Tend to bend rather than shatter when struck
Poor conductors of heat and electricity ● Tend to be either brittle solids or gases
Intermediate properties between metals and nonmetals ● Silicon - shiny like a metal, but brittle like a nonmetal.
what are orbitals
regions of space where an electron is likely to be found
e regions of space where an proton is likely to be found
e regions of space where an neutron is likely to be found
orbital is a container that can hold__electrons
2
3
4
5
Aufbau principle
Electrons fill the lowest energy orbitals first
Each orbital can have a maximum of two electrons, with opposing spins
Model in which valence electrons are represented as dots around the chemical symbol of the atom.
Pauli exclusion principle
Each orbital can have a maximum of two electrons, with opposing spins
Electrons fill the lowest energy orbitals first
Model in which valence electrons are represented as dots around the chemical symbol of the atom.
hunds rule
When filling orbitals of equal energy, electrons fill them singly first, with parallel spins
Each orbital can have a maximum of two electrons, with opposing spins
Electrons fill the lowest energy orbitals first
valence electron
Electrons in the outermost principal shell
Electrons not in the outermost principal shell
core electrons
Electrons in the outermost principal shell
Electrons not in the outermost principal shell
which two particles are located inside the nucleus
proton
neutron
electron
which particle is located outside the nucleus
proton
neutron
electron
where is all of an atoms positive charged located
proton
neutron
electron
where is all of an atoms negative choice located
proton
neutron
electron
ions
Atoms that have become charged by losing or gaining one or more electrons
have an equal number of protons and electrons
Atoms that have lost electrons and have a positive charge
Atoms that have gained electrons and have a negative charge
neutral atoms
have an equal number of protons and electrons
Atoms that have lost electrons and have a positive charge
Atoms that have gained electrons and have a negative charge.
The charge of an ion
cations
The charge of an ion
Atoms that have gained electrons and have a negative charge
Atoms that have lost electrons and have a positive charge
s have an equal number of protons and electrons
anion
Atoms that have gained electrons and have a negative charge.
Atoms that have lost electrons and have a positive charge
Atoms that have become charged by losing or gaining one or more electrons
the charge of an ion
octet rule
Atoms with eight electrons in their outermost shell are particularly stable
Small atoms, such as hydrogen, helium, and lithium, are most stable with two valence electrons
duet rule
Small atoms, such as hydrogen, helium, and lithium, are most stable with two valence electrons
Atoms with eight electrons in their outermost shell are particularly stable
Elements form ions to achieve the electron configuration of the nearest
noble gas
gas
ionic compounds are made of __ and ___
anions
cations
ions
neutral atoms
Attraction between positively-charged particles and negatively-charged particles
electrostatic attraction
electrically neutral
ionic charge
formula units
The smallest electrically-neutral collection of ions in an ionic compound
State in which all positive charges and all negative charges cancel each other out so the overall charge is 0
A group of atoms with an associated charge that acts as a single unit
electrically neutral
State in which all positive charges and all negative charges cancel each other out so the overall charge is 0
Attraction between positively-charged particles and negatively-charged particles
The smallest electrically-neutral collection of ions in an ionic compound
A group of atoms with an associated charge that acts as a single unit
polyatomic ion
monatomic ion
cations
anions
true or false polyatomic ions behave the same as monatomic ions
true
false
define molecules
Compounds that are held together by shared electrons
Bond that occurs when electrons are shared between two atoms
Molecule made of two or more atoms of the same element
Molecule made of two or more different elements
define covalent bonds
Molecule made of two or more different elements
Molecule made of two or more atoms of the same element
Bond that occurs when electrons are shared between two atoms
– Compounds that are held together by covalent bonds
true or false molecules exist as individual particles
true
false
define ionic compounds
Each formula unit is part of a large 3D array
Each molecule is an individual particle
Molecule made of two or more different elements
Bond that occurs when electrons are shared between two atoms
define molecular elements
Molecule made of two or more atoms of the same element
Molecule made of two or more different elements
Compounds that are held together by covalent bonds
– Electron pair associated with only one atom
define molecular compound
Electron pair associated with only one atom
Molecule made of two or more different elements
Molecule made of two or more atoms of the same element
Compounds that are held together by covalent bonds
In molecular compounds, electrons are (a) between atoms so that both achieve octets or duets.
VSEPR theory
A model to predict the 3-dimensional shapes of molecules
Resonance occurs when there are multiple possible Lewis structures for the same molecule
Bond that occurs when electrons are shared between two atoms
One pair of electrons shared between two atoms. Represented by a single line
Electron geometry
The arrangement of electron groups around a central atom
Arrangement of atoms around a central atom
Angle between electron charge clouds within a molecule
General term for single bonds, double bonds, triple bonds, lone pairs, and single electrons within a molecule
linear electron geometry has a __ electron groups and a bond angel of__
2
4
120
180
Trigonal Planar Electron Geometry has__electron groups and a bond angle of__
3
2
120
109.5
Tetrahedral Electron Geometry has__electron groups and a bond angel of__
4
2
120
109.5
define molecular geometry
The arrangement of atoms around a central atom
The arrangement of electron groups around a central atom
Angle between electron charge clouds within a molecule
General term for single bonds, double bonds, triple bonds, lone pairs, and single electrons within a molecule
define electronegativity
the ability of an atom to attract electrons within a covalent bond
Arrangement of electron charge clouds around a central atom
Bond that occurs when electrons are shared between two atoms
Molecule made of two or more atoms of the same element
define intermolecular forces
Attractive forces between molecules
Attractive forces between atoms
Attractive forces between electrons
Attractive forces between electron groups
dipole-dipole force
Intermolecular force between two polar molecules. The partial positive charge on one molecule is attracted to the partial negative charge on the other molecule
Hydrogen bonds occur between a hydrogen that is bonded to F, N, or O and the lone pair of electrons of an F, N, or O atom in another molecule
Intermolecular force caused by fluctuations in the electron distribution within atoms and molecules. All atoms or molecules experience London dispersion forces
hydrogen bonding
Intermolecular force caused by fluctuations in the electron distribution within atoms and molecules. All atoms or molecules experience London dispersion forces
Hydrogen bonds occur between a hydrogen that is bonded to F, N, or O and the lone pair of electrons of an F, N, or O atom in another molecule
Intermolecular force between two polar molecules. The partial positive charge on one molecule is attracted to the partial negative charge on the other molecule
London dispersion force
Intermolecular force between two polar molecules. The partial positive charge on one molecule is attracted to the partial negative charge on the other molecule
Intermolecular force caused by fluctuations in the electron distribution within atoms and molecules. All atoms or molecules experience London dispersion forces
Hydrogen bonds occur between a hydrogen that is bonded to F, N, or O and the lone pair of electrons of an F, N, or O atom in another molecule
hydrogen bond donor
A hydrogen atom bonded to F, O, or N is a hydrogen bond donor
A F, O, or N atom with an unshared pair of electrons
hydrogen bond acceptor
A F, O, or N atom with an unshared pair of electrons
A hydrogen atom bonded to F, O, or N
Occurs when matter changes state
phase change
surface tension
capillary tension
viscosity
Partial positive and partial negative charges formed by temporary, random fluctuations in electron distribution
instantaneous dipole
induced dopile
induced dipole
Partial positive and partial negative charges formed by temporary, random fluctuations in electron distribution
Partial positive and partial negative charges formed as the result of an instantaneous
what is surface tension
The tendency of liquids to minimize their surface area
Resistance of a liquid to flow
Ability of liquids to flow up a narrow tube against the force of gravity.
what is viscosity
Ability of liquids to flow up a narrow tube against the force of gravity.
Resistance of a liquid to flow
The tendency of liquids to minimize their surface area
What is Capillary Action
The tendency of liquids to minimize their surface area
Resistance of a liquid to flow
Ability of liquids to flow up a narrow tube against the force of gravity.
define chemical reaction
Atoms rearrange to form new substances
Atoms rearrange to form new molecules
Atoms rearrange to form new atoms
Atoms rearrange to form new covalent bonds
____ are the chemical(s) present before the chemical reaction takes places
reactants
products
___ are the chemical(s) present after the chemical reaction takes places
products
reactants
coefficients
Numbers placed in front of chemical formulas in a chemical equation
Numbers used in a chemical formula to indicate how many atoms or polyatomic ions are present in a molecule or formula unit
subscript
Numbers placed in front of chemical formulas in a chemical equation. Indicates the number of atoms, molecules, or formula units involved in the reaction
Numbers used in a chemical formula to indicate how many atoms or polyatomic ions are present in a molecule or formula unit
chemical changes
Chemicals are converted to different chemicals
Chemicals do not change
physical changes
Chemicals do not change
Chemicals are converted to different chemicals
oxidation reaction
Reactions in which electrons are transferred from one reagent to another
A reaction that can proceed in either direction
Reaction that changes reactants into products
A reaction in which one element displaces another within a compound
Oxidation is __ of electrons, and reduction is __ of electrons
oxidation: loss
oxidation: gain
reduction: loss
reduction: gain
reversible reactions
proceed in either direction
Reaction that changes reactants into products
Reaction that changes products into reactantt
forward reaction
Reaction that changes products into reactant
Reaction that changes reactants into product
A reaction that can proceed in either direction
reverse reaction
A reaction that can proceed in either direction
Reaction that changes reactants into products
Reaction that changes products into reactants
dynamic equilibrium
Forward and reverse reactions occur at the same rate
Describes the relative concentrations of reactants and products at equilibrium
describes the amount of chemical present
Ratio of the relative concentrations of reactants and products at equilibrium. Constant when the reaction is at a constant temperature
True or False: Reactants and products are present in equal amounts when a reaction has reached dynamic equilibrium
true
false
True or False: Nothing is happening when a system is at dynamic equilibrium
true
false
the equilibrium constant
Describes the relative concentrations of reactants and products at equilibrium
Forward and reverse reactions occur at the same rate
describes the amount of chemical present
Ratio of the relative concentrations of reactants and products when the reaction is not at equilibrium. Allows us to determine the direction in which a reaction will proceed
More reactants that products
small k
large k
More products than reactants
small k
large k
concentration
describes the amount of chemical present
Describes the relative concentrations of reactants and products at equilibrium
Forward and reverse reactions occur at the same rate
True or False: The equilibrium constant changes with temperature
true
false
molarity is a term to describe
concentration
mole
equilibrium
oxidization
reaction quotient
Ratio of the relative concentrations of reactants and products when the reaction is not at equilibrium
Ratio of the relative concentrations of reactants and products at equilibriumRatio of the relative concentrations of reactants and products at equilibrium
right towards products
Q < K
Q > K
Q = K
no change reaction is at equilibirum
Q < K
Q > K
Q = K
left towards reactants
Q < K
Q > K
Q = K
la chatelier's principle
When a chemical reaction in equilibrium is disturbed, the reaction shifts to minimize the disturbance
Ratio of the relative concentrations of reactants and products when the reaction is not at equilibrium
Ratio of the relative concentrations of reactants and products at equilibrium
How many individual items are in a mole/give Avogadro's number
(a)
True or False: It is possible to have a mole of anything: atoms, molecules, pencils, donuts…
true
false
molar mass
The mass of 1 mole of atoms, molecules, or formula units
The mass of a single molecule or formula unit, in amu
The mole is the SI unit for amount and bridges the gap between the atomic world and the everyday world
stoichometry
The relationship between quantities in a balanced chemical equation
Coefficients in a balanced chemical equation tell us the relative amounts of each chemical in a reaction
The reactant that runs out first in a chemical reaction. Determines the theoretical yield of the reaction
The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
the mole ration
The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Coefficients in a balanced chemical equation tell us the relative amounts of each chemical in a reaction
The relationship between quantities in a balanced chemical equation
The reactant that runs out first in a chemical reaction. Determines the theoretical yield of the reaction
