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AP Chemistry > Test 1 > Flashcards

Test 1 Flashcards

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1
Q

direct relationship:

A

as y increases, x increases

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2
Q

direct relationship formula

A

y=Kx

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3
Q

inverse relationship:

A

as x increases, y decreases

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4
Q

inverse relationship formula

A

y=k/x

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5
Q

exponential relationship:

A

as y increases, x increases a lot more

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6
Q

exponential relationship formula

A

y=Kx^n

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7
Q

ionization energy

A

amount of energy to remove an electron from an atom

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8
Q

Coulomb’s law(inverse square) formula

A

F= (K(Q1Q2))/(r^2)

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9
Q

use Coulomb’s law to…

A

define all trends on the periodic table

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10
Q

photoelectron spectroscopy

A

discipline of identifying unknown pure substances by using x-rays and ionization energy to produce a spectrum

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11
Q

hybridization

A

the process of orbitals hybridizing or fusing together when 2 atoms share electrons(covalent) or when 2 atoms interact with electrostatic force(ionic)

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12
Q

how to determine the hybridization of an atom

A

count number of atoms it’s bonded to and add it to the number of unshared pairs of electrons on it

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13
Q

hybridization 1

A

s

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14
Q

hybridization 2

A

sp

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15
Q

hybridization 3

A

sp^2

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16
Q

hybridization 4

A

sp^3

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17
Q

hybridization 5

A

dsp^3

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18
Q

hybridization 6

A

d^2sp^3

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19
Q

bond order

A

the number of pairs of electrons shared between 2 atoms

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20
Q

bond order single bond

A

1

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21
Q

bond order double bond

A

2

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22
Q

bond order triple bond

A

3

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23
Q

if a structure has resonance

A

take the number of bonds and divide by the number of like atoms sharing a bond

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24
Q

electronegativity

A

an atoms ability to attract electrons to itself

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25
Q

electronegativity trend

A

up and to the right

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26
Q

intramolecular bond

A

bond between atoms

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27
Q

three types of intramolecular bonds

A

ionic, covalent, polar covalent

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28
Q

polar molecule

A

molecule with uneven charges because the atoms have different electronegativity values

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29
Q

dipole

A

having opposites charged ends

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30
Q

if a molecule is diatomic and

A

the bond between the atoms is polar, then the molecule itself is polar

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31
Q

if a molecule has more than 2 atoms

A

the polarity of the bond and the 3-D shape must be considered

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32
Q

if the dipoles go in opposite directions

A

they cancel each other out forming a non polar molecule

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33
Q

intermolecular forces

A

weak interaction between molecules in liquids and solids

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34
Q

intermolecular forces are responsible for

A

1.solids and liquids staying together
2.boiling point, melting point, solubility, and vapor pressure

35
Q

IMFs from strongest to weakest

A

ion-dipole, H bonding, dipole-dipole, london dispersion forces(LDFs)

36
Q

ion-dipole

A

interaction between an ion(dissolved salt) and a polar molecule

37
Q

water molecules surround the ions forming

A

hydration shells

38
Q

H bonding(hydrogen bonding)

A

interaction between the hydrogen of one molecule and the F O or N

39
Q

dipole-dipole

A

the positive end of a polar molecule interacts with the negative end of another molecule

40
Q

london dispersion forces(LDFs)

A

weakest IMF that both polar and non-polar molecules have

41
Q

if non-polar substances collide

A

causing a temporary induced dipole that causes more interaction

42
Q

the larger the atom

A

the stronger the dispersion forces

43
Q

5 types of reactions

A

synthesis, decomposition, combustion, single displacement, and double displacement

44
Q

neutralization reaction

A

reaction that is exothermic when an acid is combined with a base producing a salt and water

45
Q

precipitation reaction

A

reaction that forms an insoluble solid(precipitate) from the mixing of 2 aqueous solutions

46
Q

ap solubility rule

A

salts made with group 1A elements, ammonium(NH4), and nitrate are soluble

47
Q

ammonium hydroxide

A

NH4OH -> NH3 + H2O

48
Q

carbonic acid

A

H2CO3 -> CO2 + H2O

49
Q

dissociation

A

process of separating positive ions from negative ions in a polar solvent

50
Q

complete ionic equation

A

balanced chemical equation where soluble salts are expressed in their dissociated state and insoluble salts are expressed in their associated state

51
Q

spectator ions

A

ions that are present on both sides of a chemical equation that don’t participate in a chemical reaction

52
Q

net ionic equation

A

balanced equation once the spectator ions have been removed

53
Q

1st law of thermodynamics

A

energy cannot be created nor destroyed; only converted from one form to another

54
Q

enthalpy

A

change in the heat content of a system from a reaction or phase change

55
Q

+ delta H

A

endothermic reaction

56
Q

-delta H

A

exothermic reaction

57
Q

delta H notation

A

placing the value for enthalpy beside a balanced chemical equation

58
Q

thermochemical notation

A

the enthalpy value is incorporated into the balanced equation

59
Q

Hess’s law(law of heat summation)

A

the enthalpy value for a chemical reaction is equal to the sum of the enthalpy values of the reactions that make up the reaction

60
Q

which sign of enthalpy is thermodynamically favored

A

-deltaH

61
Q

standard enthalpy of formation of the reaction=

A

the standard enthalpy of the products - reactants

62
Q

specific heat equation

A

q=cxmxdeltaT

63
Q

entropy(s)

A

measurement of disorder in a system; measured in J/K or J/K(mol)

64
Q

entropy is not a

A

measurement of energy but how energy is dispersed

65
Q

2nd law of thermodynamics

A

entropy increases in a closed system

66
Q

which entropy is thermodynamically favored

A

+deltas

67
Q

microstate

A

all the possible positions that particles can occupy at a particular time

68
Q

entropy can increase when ___ increases

A

microstates, electrons, and atoms in cmpd

69
Q

Boltzmann equation

A

s=Kb(ln(W))

70
Q

Boltzmann’s constant

A

1.38 x 10^-23 J/K

71
Q

3rd law of thermodynamics

A

the entropy of a pure crystal at absolute zero is zero(only one micro state is possible. the ln(1)=0)

72
Q

positional disorder

A

based on the position of particles(microstates)

73
Q

thermal disorder

A

dispersion of heat and energy( increased temperature, increased entropy)

74
Q

delta entropy=

A

entropy of the system + entropy of the surroundings

75
Q

entropy of surroundings=

A

-deltaH(1000)/T

76
Q

entropy of system=

A

delta H/T

77
Q

standard entropy of formation=

A

standard entropy of formation of the products - reactants

78
Q

gibbs free energy

A

third thermodynamic quantity measured in kJ/mol that is defined as the energy available to do work in a system

79
Q

thermodynamically favored gibbs free energy

A

-delta G

80
Q

Gibbs-Hemholtz Equation

A

deltaG= deltaH - T(deltaS)
temp in K
covert entropy delta S to kJ

81
Q

bond energy(BE)

A

energy required to break a bond in 1 mole of a gaseous molecule

82
Q

bond energy requirements

A

-gaseous products and reactants
-values are experimentally determined
-units in kJ
-known lewis structure

83
Q

bond energy=

A

sum of reactants - products

AP Chemistry (16 decks)

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