1
Q
What is matter?
A
Anything that has mass and volume
2
Q
What are the two main classifications of matter?
A
Pure substances and mixtures
3
Q
What are the two types of pure substances?
A
Elements and compounds
4
Q
What is a homogeneous mixture?
A
A mixture with uniform composition
5
Q
What is a heterogeneous mixture?
A
A mixture with non-uniform composition
6
Q
What is a physical property?
A
A property observed without changing composition
7
Q
What is a chemical property?
A
A property describing ability to undergo chemical change
8
Q
What is density?
A
Mass per unit volume
9
Q
Density formula?
A
density = mass / volume
10
Q
What is the base unit of mass in the metric system?
A
gram (g)
11
Q
What is the base unit of volume in the metric system?
A
liter (L)
12
Q
What is the base unit of length in the metric system?
A
meter (m)
13
Q
What does kilo- mean?
A
10^3
14
Q
What does milli- mean?
A
10^-3
15
Q
What are significant figures?
A
Digits known with certainty plus one estimated digit
16
Q
Do leading zeros count as sig figs?
A
No
17
Q
Do trailing zeros count as sig figs?
A
Only if a decimal is present
18
Q
What is dimensional analysis?
A
Unit conversion using conversion factors
19
Q
What is an atom?
A
The smallest unit of an element
20
Q
What is atomic number?
A
Number of protons
21
Q
What is mass number?
A
Protons + neutrons
22
Q
What is atomic weight?
A
Weighted average of isotopic masses
23
Q
What is an isotope?
A
Atoms of same element with different neutrons
24
Q
What do periods represent?
A
Rows on the periodic table
25
What do groups represent?
Columns with similar properties
26
What defines an ionic compound?
Electron transfer between metal and nonmetal
27
What defines a molecular compound?
Electron sharing between nonmetals
28
What charge do Group 1 metals form?
1
29
What charge do Group 2 metals form?
2
30
What charge do halogens form?
-1
31
What is a polyatomic ion?
A charged group of covalently bonded atoms
32
What is the goal when forming ionic formulas?
Total charge equals zero
33
How do you name ionic compounds?
Cation name + anion name
34
How do you name acids ending in -ide?
hydro-___-ic acid
35
How do you name acids ending in -ate?
___-ic acid
36
How do you name acids ending in -ite?
___-ous acid
37
What is a chemical equation?
A symbolic representation of a chemical reaction
38
What must be conserved when balancing equations?
Atoms
39
What is a synthesis reaction?
Two or more substances form one product
40
What is a decomposition reaction?
One compound breaks into simpler substances
41
What is a single replacement reaction?
One element replaces another
42
What is a double replacement reaction?
Exchange of ions between compounds
43
What is molar mass?
Mass of one mole of a substance
44
What is percent composition?
Percent by mass of each element in a compound
45
Percent composition formula?
(mass of element / total mass) × 100
46
What is a mole?
6.022 × 10^23 particles
47
What is Avogadro’s number?
6.022 × 10^23
48
How do you convert grams to moles?
Divide by molar mass
49
How do you convert moles to particles?
Multiply by Avogadro’s number
50
How do subscripts affect mole calculations?
They indicate ratios of atoms or ions
51
Steps to find empirical formula from mass?
Convert g→mol
52
What is stoichiometry?
Calculations using balanced equations
53
What is a limiting reactant?
Reactant consumed first
54
What is percent yield?
Measure of reaction efficiency
55
Percent yield formula?
(actual / theoretical) × 100
56
What is a strong electrolyte?
Completely dissociates into ions
57
What is a weak electrolyte?
Partially ionizes in water
58
What is a nonelectrolyte?
Does not form ions
59
What is a molecular equation?
Shows compounds as intact molecules
60
What is an ionic equation?
Shows dissociated ions
61
What is a net ionic equation?
Spectator ions removed
62
What is a precipitation reaction?
Formation of an insoluble solid
63
What defines an acid (Arrhenius)?
Produces H+ in water
64
What defines a base (Arrhenius)?
Produces OH- in water
65
What is a neutralization reaction?
Acid + base → salt + water
66
What is oxidation?
Loss of electrons
67
What is reduction?
Gain of electrons
68
What happens to oxidation number during oxidation?
It increases
69
What is the activity series used for?
Predicting single replacement reactions
70
What is molarity?
Moles of solute per liter of solution
71
Molarity formula?
M = mol / L
72
What is the dilution formula?
M1V1 = M2V2
73
What is a titration?
Controlled reaction to determine concentration
74
What is energy?
Capacity to do work or transfer heat
75
First law of thermodynamics?
Energy is conserved
76
ΔE equation?
ΔE = q + w
77
What does q represent?
Heat
78
What does w represent?
Work
79
What is an endothermic process?
Absorbs heat (q > 0)
80
What is an exothermic process?
Releases heat (q < 0)
81
What is a state function?
Depends only on initial and final states
82
What is enthalpy?
Heat content at constant pressure
83
What is Hess’s Law?
ΔH depends only on initial and final states
84
Calorimetry heat equation?
q = mcΔT
85
What does specific heat measure?
Resistance to temperature change
86
How do you calculate ΔH from formation enthalpies?
Σproducts − Σreactants
87
Bond enthalpy method for ΔH?
Bonds broken − bonds formed
88
Energy of a photon equation?
E = hν
89
Relationship between wavelength and frequency?
c = λν
90
What is a line spectrum?
Discrete emission lines of atoms
91
What model explains hydrogen spectra?
Bohr model
92
What are orbitals?
Regions of high electron probability
93
What is Pauli exclusion principle?
No two electrons have same 4 quantum numbers
94
What is Hund’s rule?
Electrons occupy orbitals singly first
95
What is effective nuclear charge?
Net positive charge felt by valence electrons
96
Trend for atomic radius across a period?
Decreases
97
Trend for atomic radius down a group?
Increases
98
Trend for ionization energy across a period?
Increases
99
Trend for electron affinity across a period?
Becomes more negative
100
What do Lewis symbols represent?
Valence electrons
101
How do you form cations?
Lose electrons
102
How do you form anions?
Gain electrons
103
What increases lattice energy?
Higher charge and smaller ions
104
What is bond enthalpy?
Energy required to break a bond
105
What is the octet rule?
Atoms tend to have 8 valence electrons
106
Formal charge formula?
Valence − (lone + 1/2 bonding)
107
What determines bond polarity?
Electronegativity difference
108
What theory predicts molecular shape?
VSEPR
109
What causes deviations in bond angles?
Lone pairs
110
What determines molecular polarity?
Shape + bond polarity
111
What is resonance?
Multiple valid Lewis structures
112
What is hybridization?
Mixing of atomic orbitals
113
Hybridization for tetrahedral?
sp3
114
Hybridization for trigonal planar?
sp2
115
Hybridization for linear?
sp
116
What is a sigma bond?
Head-on orbital overlap
117
What is a pi bond?
Side-by-side orbital overlap
118
What state of matter has variable shape and volume?
Gas
119
What is pressure?
Force per unit area
120
Boyle’s Law relationship?
P ∝ 1/V
121
Charles’s Law relationship?
V ∝ T
122
Avogadro’s Law relationship?
V ∝ n
123
Ideal Gas Law?
PV = nRT
124
What does Dalton’s Law describe?
Partial pressures
125
Partial pressure formula?
Ptotal = ΣPi
126
What does Kinetic Molecular Theory state?
Gas particles move constantly
127
What increases molecular speed?
Higher temperature
128
What causes real gas behavior?
High pressure or low temperature
129
What are intermolecular forces?
Attractions between molecules
130
Strongest IMF listed here?
Ion-dipole
131
What causes London dispersion forces?
Temporary dipoles
132
What defines hydrogen bonding?
H bonded to N
133
What is vapor pressure?
Pressure of vapor above liquid
134
How does temperature affect vapor pressure?
Higher T → higher vapor pressure
Chemistry 1210
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