Studied by 2 peopledecomposition
AB → A + B
Single Displacement
Element + Compound → Compound + Element
(A + BC → AC + B)
(Zn + H2SO4 → ZnSO4 + H2)
Ionic bonds
transfer of electrons
Covalent bonds
sharing of electrons
Anion
negative ions
more negative because they gain electrons
nonmetals
end in -ide
Cation
Positive ions
more positive because the lose electrons
metals
Octet Rule definition
atoms tend to gain, lose, or share electrons in order to acquire eight valence electrons (noble gas configurations)
Non-metals tend to
gain electrons
Metals tend to
lose electrons
When two elements transfer electrons
Ionic bond is formed
Diatomic Molecules
N2, H2, O2, Cl2, F2, Br2, I2,
forms a seven on the periodic table
atoms are chemically bonded
exist in nature
two of the same types of atoms
Alkali metals & Alkaline Earth Metals bond with
Halogens
Oxides
A metal forms a bond with oxygen
Binary Compounds
two elements
Monatomic
containing one atom
Polyatomic ions
Composed of more than two elements
Salt is formed
A non-metal and a metal
Properties of Ionic compounds
hard but brittle
high boiling and melting points
Solids dont conduct electricity
Liquids/Solutions conduct electricity
Diatomic molecules bond
Diatomic covalent bonding
Water
polar covalent compound
oxygen has six valence electrons
each hydrogen atom has one valence electron
Types of Covalent Bonds
Single Bonds, Double Bonds, Triple Bonds
SIngle Bond
atoms share one pair of electrons (2)
Double Bonds
atoms share two pairs of electrons (4)
Triple Bonds
atoms share three pairs of electrons (6)
Lewis structures show
arrangements of electrons and bond
Strenght of a covalent bond is dependent on
bond length
Bond Length
the distance between two bonded nuclei
Bond-Dissociation energy
amount of energy needed to break bonds
Inverse relationship between bond length and bond energy
Conversion for temperature (SI Unit)
273° K = 0° C
Lewis structures can predict
molecular shape
Unshared pairs of electrons can influence
molecular shape
Molecular orbital
the region of high probability that is occupied by an individual electron as it travels with the wavelike motion in the three-dimensional space around one of two or more associated nuclei
Dipole
has a slight negative and positive end
The symbol 𝛿
shows partial negative or partial positive charge
Electronegativity
determines Bond Type
Polarity
related to Bond Strength
Reactions occur when
substances undergo changes
Bonds are ____, and new bonds are ____ in a chemical reaction
broken, formed
Combustion reactions always have
Water (H2O) and Carbon Dioxide (CO2) on the product side
△
heat has been added
Products
substances formed by reaction
right of the arrow
States of matter
(s), (l), (g), or (aq)
Evidence of a Chemical Change
color change
evolution of a gas
formation of a precipitate
release or absorption of energy
Endothermic
absorption of heat
exothermic
release of heat
What is the study of quantitative relationships between the amount of reactants used and the amounts of products formed by a chemical reaction
Stoichiometry
Percent Yield
Percent Yield = (Actual Yield / Theoretical Yield ) x 100
Stoichiometry is based on the law of. . .?
Conservation of mass
When atoms or ions are used in an equation what conversion factor must be used?
Avogadro’s Constant
What is always the first step in a stoichiometry problem
The given
Double Displacement
Compound + Compound → Compound + Compound
(AD+ BC → AC + BD)
(AgNO3 + NaCl → AgCl + NaNO3)
(*metals go with nonmetals*)
Combustion
compound/elements + O2 → products
(CH4 + O2 → CO2 + H2O)
Synthesis
A + B → AB
(Zn +I2 → ZnI2)
1
mono
6
hexa
0.5 - 2.1
polar covalent
Linear
Trigonal Pyramidal
Which atom is most likely to form a triple covalent bond
Carbon
Bent
Tetrahedral
2
di
3
tri
4
tetra
5
penta
7
hepta
8
octa
9
nona
10
deca
Covalent bonds are between
two nonmetals
Bonds lengths ______ distances because bonds are ______
average, rigid
A gaseous substance with poor conductivity is most likely a(n) ________________.
A non-metal/molecular compound
Pt symbol
a catalyst
Ag(s) + NaCl(aq) →
Na(s) + AgCl(aq)
SI unit for amount
Mole/Mol
A mole is
the number of atoms in exactly 12 grams of carbon-12
number of particle in a mole is called
Avogadro’s Number
(6.022 x 10^23)
Mole ratio
the key in Stoichiometry
Mole ratio is
a ratio between the number of moles of any two substance in a balanced chemical equation
limiting reactant
determines the amount of product formed
determines the theoretical yield
the one that runs out first
excess reactant
the reactant that is left over
Theoretical Yield
the maximum amount of product that can be formed from a given reactant
Theoretical Yield is higher than actual yield
Actual Yield
the amount of product produced in a chemical experiment
Percent Yield
the ratio of actual yield to theoretical yield
describes the efficiency of a reaction
Precent Yield formula
Percent yield = actual/theoretical x 100
Coefficients in a chemical equations are used in which one of the following conversion factors?
mole ratios
In stoichiometric calculations, you should:
round off only the final answer
Boyle’s law
inverse relationship between volume and pressure
“volume of a fixed amount of gas at constant temperature varies inversely with pressure”
P1V1 = P2V2
As volume increases
pressure decreases
As volume decreamses
pressure increases
Charles’ Law
Direct relationship between volume and temperature
“the volume of a given amount of gas is directly proportional to the Kelvin temperature
V1/T1 = V2/T2
As temperature increases
volume increases
As temperature decreases,
volume decreases
0° Celsius
273° Kelvin
uses for all v/t equations
used in p/t problems
Gay-Lussac’s law
Direct relationship between pressure and temperature
“The pressure of a fixed amount of gas varies directly with Kelvin temperature when volume remains constant”
P1/T1 = P2/T2 OR P/T = K
As temperature increases
pressure increases
As temperature decreases
pressure decreases
Which is not a unit which describes pressure?
Newton
Finding the Percent of an Element in a Compound Formula
element/compound x 100
Triagonal Planar
Note 
Flashcard (30)