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WorksheetsFacts I need to Memorize
Total questions: 105
Worksheet time: 4hrs 30mins
Protons are
positively charge
mass of 1 amu
Neutrons
have no charge
have a mass of 1 amu
are negatively charged
Electrons
small with a mass of 1/2000 amu
negatively charge
positively charged
Nucleus of the atom
is positive
is surrounded by negatively charged electrons
is surrounded by negatively charged protons
number of protons
equals number of electrons
identifies an element
mass of protons equals
mass of electrons
mass of neutrons
particle arrangement means
how the particles are bounded to each other
CO2 and C2O, for example, have different particle arrangement
Metals
are good conductors of electricity
do not conduct electricity
are malleable
A number after the element, like C-14 is the
mass number
number of protons
Elements that have atoms with stable valence electron configurations in the ground state are found in
Group 1
Group 3
Group 18
When an atom loses an electron
it becomes positive and a smaller radius
it becomes negative and a bigger radius
An atom of which an element has the strongest attraction for the electrons
is closer to having 8 valence electrons
is closer to having no valence electrons
Electrons are in the
orbitals
nucleus
mass number
atom’s number of protons and neutrons added together
just number of protons
same structural but different molecular formula
Atomic number
the number of protons in the nucleus of an atom
the number of neutrons in the nucleus of an atom
number of neutrons
mass number – atomic number.
number of electrons-number of protons
In a neutral atom
number of protons = the number of electrons.
number of protons = the number of neutrons
Isotopes
equal numbers of protons, but differ in their neutron numbers
same molecular structure but different structural formula
Positive ions
when a neutral atom loses electrons
They are smaller than the neutral atom
when a neutral atom gains electrons
negative ions
form when a neutral atom gains electrons
They are larger than the neutral atom
form when a neutral atom loses electrons
Ernest Rutherford’s gold foil experiment showed that
an atom is mostly empty space
there is small, dense, positively charged nucleus.
there is an orbital
J.J. Thompson discovered
the electron
the “plum-pudding” model of the atom.
the orbital
Bohr Model of the atom
placed electrons in “planet-like” orbits around the nucleus of an atom.
created the plum pudding model
wave-mechanical model of the atom
has electrons in “clouds” (orbitals) around the nucleus
has electrons in the nucleus
Bright line spectra are produced when
electrons emit energy as light when they fall from higher energy levels back down to lower (ground state) energy levels
electrons emit energy as light when they move from lower energy levels (ground state) to higher energy levels
Elements
pure substances
composed of atoms with the same atomic number
They cannot be decomposed
Diatomic molecules
elements that form two atom molecules in their natural form at STP
elements that form three atom molecules in their natural form at STP
How many significant figures are in number value: 3043
5
4
3
How many significant figures are in number value: 0.0000042
7
6
2
3
How many significant figures are in number value: 8.50
2
3
In terms of significant figures, when multiplying or dividing measurements, final answer must have
as many digits as the measurement with the fewest number of significant figures.
as many digits as the measurement with the highest number of significant figures.
homogeneous mixtures are
solutions
particles are evenly distributed
one layer
Heterogeneous mixtures
particles are unevenly distributed
two layers
solute
substance being dissolved (ice tea powder)
substance that dissolves the solute (water)
Isotopes could be written as
C-14
Carbon-14
average atomic mass
weighted average mass of all the naturally known isotopes of an element
weighted average mass of all the artificial known isotopes of an element
electron configuration
The distribution of electrons in an atom
found on the periodic table
outermost electrons
valence electrons
determine the chemical properties
found on periodic table at the bottom of every element
empirical formula
simplest mole ratio among the elements in a compound
same as molecular formula
Ex: CH2
Lewis dot model
way of representing the valence electron of an atom
way of representing protons around an atom
Polyatomic ions
Found on Table E
covalently bonded together
have an overall charge
Coefficients
in front of the formulas of reactants and products to balance chemical equations
subscripts of every atom
When naming ionic compounds
write the name of the positive ion first, followed by the name of the negative ion (anion)
change the name ending to “-ide.”
When naming compounds containing polyatomic ions
keep the name of the polyatomic ion the same as it is written in Table E.
change the name of the polyatomic ion to "-ide"
Roman numerals are used
to show the positive oxidation number of the metal if it has more than one positive oxidation number
to show the oxidation number of the nonmetal
Physical changes
do not form new substances.
They merely change the appearance of the original material. Ex: H2O (s) --> H2O (l)
Chemical changes
result in the formation of new substances
Ex: combustion
Reactants
on the left side of the reaction arrow
chemicals USED in a chemical reaction
chemicals produced in a chemical reaction
Temperature
measure of average kinetic energy
measure of average potential energy
Exothermic reactions
release energy (energy is a product of the reaction)
absorb energy (energy is a reactant of the reaction)
when balancing equations
coefficients change
subscripts change
Synthesis reactions
two or more reactants combine to form a single product
a single reactant forms two or more products
Decomposition reactions
when a single reactant forms two or more products
when two or more reactants combine to form a single product
Single replacement reactions
one element replaces another element in a compound.
two compounds react to form two new compounds
Double replacement reactions
two compounds react to form two new compounds
one element replaces another element in a compound
Law of Conservation of Mass and Energy
masses (and energy and charge) of the reactants in a chemical equation is always equal to the masses (and energy and charge) of the products
protons - neutrons = electrons
masses of the reactants have to be multiplied by the subscripts
gram formula mass (molar mass)
sum of the atomic masses of all the atoms in it
sum of the atomic numbers of all the atoms in it
percentage composition of a compound
formula is on table T
formula is on table S
Equal volumes of gases, pressure and temperature
means equal number of molecules
means equal number of atoms
to convert molecular formula into empirical formula
divide by the common multiple of all the subscripts
multiply the coefficients
kinetic molecular theory
particles are “small spheres” with negligible (virtually no) volume
particles move in a straight-line path random motion
particles in a solid
rigidly held together, closely packed
crystal structure
Liquids
have no definite shape
have a definite volume.
Gases
widely-spaced particles that are in random motion
no definite shape or volume
sublime
solid--> gas
gas --> solid
liquid--> gas
As temperature increases,
vapor pressure increases.
vapor pressure decreases
“STP”
Standard Temperature and Pressure
found on table A
Degrees Kelvin
= °C + 273
measurement of volume
conversion found on Table S
conversion found on Table T
Heat is a transfer of energy from
higher temperature to one at lower temperature
lower temperature to one at higher temperature
In q = mCΔt , the C value is the
specific heat capacity
found on Table B for water
= 334 J/g
heat of fusion
heat absorbed or released when 1 gram of a substance changes between the solid and liquid phases
key words to look for: freeze or melt
334 J/g for water
heat of vaporization
heat absorbed or released when 1 gram of a substance changes between the liquid and gaseous phases
key words to look for: vaporize, boil, or condense
For the combined gas law equation
use Kelvins for the temperature
use Celsius for the temperature
As the pressure exerted on a gas increases
the volume decreases proportionally.
the volume increases proportionally.
As the pressure on a gas increases
temperature increases.
temperature decreases
the temperature of a gas increases
volume increases.
volume decreases
Real gas particles
have volume
are attracted to one another
Real gases behave more like ideal gases
low pressures and high temperatures.
high pressures and low temperatures.
Mixtures may be separated by several physical means
True
False
Distillation
separates mixtures with different boiling points.
separates mixtures of solids and liquids.
Filtration
separates mixtures of solids and liquids.
separates mixtures with different boiling points.
Chromatography
used to separate mixtures of liquids and mixtures of gases
separates mixtures with different boiling points.
Periods
horizontal rows on the Periodic Table
vertical columns on the Periodic Table
Groups
vertical columns on the Periodic Table.
horizontal rows on the Periodic Table.
Metals
found left of the “staircase” on the Periodic Table
malleable
ductile
conduct electricity
Noble gases (Group 18)
unreactive
stable due to the fact that their valence level of electrons is completely filled.
have 8 valence electrons
are metals
Ionization energy
found on table S
found on table T
Atomic radii decrease left to right across a period
due to increasing nuclear charge
due to more valence electrons
Atomic radii increase as you go down a group
due to increased electron energy levels
due to decreased electron energy levels
Electronegativity
measure of an element’s attraction for electrons.
measure of an protons’s attraction for electrons.
measure of how much energy needed to remove an electron
Electronegativity ______________ as you go up and to the right on the Periodic Table.
increases
decreases
The elements in Group 17 are
the halogens.
the noble gases
Energy is absorbed when a chemical bond
breaks
forms
last digit of an electron configuration
is the number of valence electrons
atomic number
Metallic bonds
sea of electrons
between metals
Ex:Cu (s)
octet rule
most stable when elements have 8 valence electrons
most stable when elements have 1 valence electrons
Covalent bonds
form when two atoms share a pair of electrons
form when two metals share electrons
form between nonmetals
Ionic bonds
one atom transfers an electron to another atom when forming a bond with it
one atom shares an electron to another atom when forming a bond with it
Nonpolar covalent bonds
atoms of same element bond together
equal share of electrons
symmetrical
Polar covalent bonds
asymmetrical
different elements
unequal charge distribution
molecular substances
Substances containing mostly covalent bonds
substances containing ionic bonds
Hydrogen bonds
attractive forces that form when hydrogen bonds to the elements N, O, or F
between hydrogen and hydrogen
water
is polar
dissolves polar molecules
is nonpolar
Like dissolves like
polar dissolves polar molecules
nonpolar dissolves nonpolar
As temperature increases
solubility increases for most solids.
solubility increases for most solids.
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