UNIT I Flashcards
(131 cards)
1
Q
Study of hydrocarbons and their various derivatives
A
Organic chemistry
2
Q
Study of all substances other than hydrocarbons and their derivatives
A
Inorganic chemistry
3
Q
number of inorganic compounds
A
1.7 million
4
Q
number of organic compounds
A
10 million
5
Q
Compounds are categorized into two types:
A
organic compounds, inorganic compounds
6
Q
from living organisms (with a vital force)
A
organic compounds
7
Q
from minerals (without a vital force)
A
inorganic compounds
8
Q
organic chemistry = compounds that contain ______
A
carbon
9
Q
is a compound made from carbon atoms
A
organic compound
10
Q
has one or more C atoms
A
organic compound
11
Q
has many H atoms
A
organic compound
12
Q
may also contain O, S, N, P, and halogens
A
organic compound
13
Q
Properties of Organic Compounds
A
• contain carbon
• have covalent bonds
• have low melting points
• have low boiling points
• are flammable
• are soluble in nonpolar solvents
• are not soluble in water
14
Q
______, ______, is an organic compound used
as a fuel.
A
Propane, C3H8
15
Q
______, ______, is an inorganic compound composed of Na+ and Cl– ions.
A
NaCl, salt
16
Q
Identify each of the following characteristics as most
typical of compounds that are I) inorganic or O) organic.
has a high melting point
A
I
17
Q
Identify each of the following characteristics as most
typical of compounds that are I) inorganic or O)
organic.
is not soluble in water
A
O
18
Q
Identify each of the following characteristics as most
typical of compounds that are I) inorganic or O)
organic.
has a formula CH3─CH2─CH3
A
O
19
Q
Identify each of the following characteristics as most
typical of compounds that are I) inorganic or O)
organic.
has a formula MgCl2
A
I
20
Q
Identify each of the following characteristics as most
typical of compounds that are I) inorganic or O)
organic.
burns easily in air
A
O
21
Q
Identify each of the following characteristics as most
typical of compounds that are I) inorganic or O)
organic.
has covalent bonds
A
O
22
Q
Atoms to the left of carbon ______ electrons.
A
give up
23
Q
Atoms to the right of carbon ______ electrons.
A
accept
24
Q
Carbon ______ electrons.
A
shares
25
In carbon compounds, carbon has ______ valence electrons, and hydrogen has ______
4, 1
26
to achieve an octet, C forms ______ bonds
four
27
Carbon (C) atom makes total ______ bonds
4
28
The sharing of four valence electrons requires the
formation of four ______ which are represented by four lines
covalent bonds
29
______ predicts that a carbon atom with four single, covalent bonds is tetrahedral as shown in a
(a) tetrahedron
(b) ball-and-stick model
(c) space-filling model
(d) expanded structural
formula
VSEPR theory
30
In organic molecules with more carbon atoms, ______ electrons are shared
valence
31
In organic molecules with more carbon atoms, ______ bonds form between carbon and carbon atoms
covalent
32
In organic molecules with more carbon atoms, ______ bonds form between carbon and hydrogen atoms
covalent
33
______ are positively charged.
Protons
34
______ have no charge.
Neutrons
35
______ are negatively charged.
Electrons
36
Atomic number = # of ______
protons
37
Atomic number of carbon = ______
6
38
Neutral carbon has six ______ and six ______.
protons, electrons
39
number of protons + number of neutrons = ______
mass number
40
mass number - number of protons = ______
number of neutrons
41
______ = number of protons – number of electrons
charge of an ion
42
have the same atomic number, but different mass numbers
isotopes
43
All carbon atoms have the same atomic number, but not all have the same mass number because they do not all have the same number of ______.
neutrons
44
The first shell is ______ to the nucleus.
closest
45
The closer the atomic orbital is to the nucleus, the ______ its energy.
lower
46
Mnemonics of electron distribution
ELECTRON CONFIGURATION
47
Describes the arrangement of electrons by sublevel
according to increasing energy
ELECTRON CONFIGURATION
48
An electron goes into the atomic orbital with the lowest energy.
Aufbau principle
49
No more than two electrons can be in an atomic
orbital; the two electrons must be of opposite spin.
Pauli exclusion principle
50
An electron goes into an empty degenerate orbital rather than pairing up.
Hund’s rule
51
______ electronic configuration of an atom describes the orbitals occupied by the atom’s electrons when they are all in the available orbitals with the lowest energy.
Ground-state
52
______ electronic configuration results when energy is applied to an atom in the ground state, one or more electrons can jump into a higher-energy orbital. The atom then would be in an excited state.
Excited-state
53
______ are electrons in inner shells (those below the outermost shell). They do not participate in chemical bonding.
Core electrons
54
______ are electrons in the outermost shell.
Valence electrons
55
Accounts for the outermost or valence electrons of an atom.
Condensed Electron Configurations
56
The electron configuration can be abbreviated by indicating the innermost electrons with the symbol of the corresponding noble gas.
Condensed Electron Configurations
57
Number of valence electrons = ______ number
Group
58
______ developed a method to denote potential
bonding electrons by using one dot for every valence electron around the element symbol.
G. N. Lewis
59
When forming compounds, atoms tend to gain, lose, or share electrons until they are surrounded by eight valence electrons (the ______).
octet rule
60
Atoms on the Left Side of the Periodic Table ______ an Electron
Lose
61
Atoms on the Right Side of the Periodic Table ______ an Electron
Gain
62
A ______ Atom Can Lose or Gain an Electron
Hydrogen
63
An ______ is Formed by the Attraction Between Ions of Opposite Charge
Ionic Bond
64
______ are Formed by Sharing Electrons
Covalent Bonds
65
Nonpolar covalent bond = bonded atoms are ______
the same
66
Polar covalent bond = bonded atoms are ______
different
67
Bond polarity depends on the ______ in ______.
difference, electronegativity
68
Difference in electronegativity is a gauge of ______.
bond polarity
69
If the electronegativity difference between two bonded atoms is 0.4-1.9 (unequal sharing of electrons)
Polar Covalent Bond
70
If the electronegativity difference is >2.0 (transfer of electrons)
Ionic Bond
71
If the electronegativity difference is 0-0.39 (equal sharing of electrons)
Nonpolar Covalent Bond
72
the greater the difference in electronegativity, the ______ the dipole moment, and the ______ polar the bond
greater, more
73
Formal charge formula
FC = VE - (B +d)
74
In order to have a complete octet, the number of bonds and the number of lone pairs must total ______.
four
75
An ______ is a three-dimensional region around the nucleus where an electron is most likely to be found.
atomic orbital
76
______ orbital is a sphere with the nucleus at its center.
s
77
______ have both particle-like and wave-like properties.
Electrons
78
A ______ is a consequence of the wave-like properties of an electron.
node
79
There is zero probability of finding an electron at the ______.
node
80
p orbitals have ______ lobes. They are generally depicted as ______ shaped. Computer-generated representations reveal that they are more like ______.
two, teardrop, doorknobs
81
______ node (node): A point or plane of zero electron density in an orbital. Always bordered by two or more orbital lobes.
Orbital
82
Three p orbitals have ______ energy.
the same
83
Each p orbital is ______ to the other two p orbitals.
perpendicular
84
______ combines the tendency of atoms to fill their octets by sharing electrons (the Lewis model) with their wavelike properties, assigning electrons to a volume of space called an orbital.
Molecular orbital (MO) theory
85
According to MO theory, covalent bonds result when
atomic orbitals combine to form ______.
molecular orbitals
86
The covalent bond that is formed when the two orbitals overlap is called a ______ bond.
sigma (σ)
87
Orbitals are ______. The number of molecular orbitals formed must equal the number of atomic orbitals combined.
conserved
88
We think of covalent bonds forming through the
sharing of electrons by adjacent atoms. In such an approach this can only occur when orbitals on the two atoms ______.
overlap
89
______ bonds are characterized by
• Side-to-side overlap.
• Electron density above and below the internuclear axis.
Pi
90
The four C-H bonds in methane are identical because carbon uses ______ atomic orbitals.
hybrid
91
An ______ orbital has a large lobe and a small lobe.
sp3
92
______ are mixed orbitals that result from combining atomic orbitals.
Hybrid orbitals
93
Carbon is tetrahedral. The tetrahedral bond angle is ______.
109.5°
94
All the bonds in methane and ethane are ______. All single bonds in organic compounds are ______.
sigma (s) bonds
95
The Two sp Orbitals Point in ______ Directions. The Two p Orbitals are ______.
Opposite, Perpendicular
96
orbitals used in bond formation determine the ______
bond angle
97
The shorter the bond, the ______ it is.
stronger
98
A π Bond is ______ Than a σ Bond
Weaker
99
Hydrogen-containing compound that produces H+ ions in solution
Arrhenius acid
100
Hydroxide-containing compound that produces OH– ions in solution
Arrhenius base
101
Substance that can donate a proton (H+ ion) to some other substance
̶ Proton donor
Brønsted–Lowry acid
102
Substance that can accept a proton (H+ ion) from some other substance
̶ Proton acceptor
Brønsted–Lowry base
103
When an acid loses a proton, it forms its ______.
conjugate base
104
When a base gains a proton, it forms its ______.
conjugate acid
105
A substance that can either lose or accept a proton
and thus can function as either a Brønsted–Lowry
acid or a Brønsted–Lowry base
Amphiprotic Substance
106
An acid that supplies one proton (H+ ion) per molecule during an acid–base reaction
Monoprotic Acid
107
An acid that supplies two protons (H+ ions) per
molecule during an acid–base reaction
Diprotic Acid
108
Carbonic acid (H2CO3) is a ______ acid
diprotic
109
An acid that supplies three protons (H+ ions) per
molecule during an acid–base reaction
Triprotic Acid
110
______ acid, ______, is the most common triprotic acid.
Phosphoric, H3PO4
111
An acid that supplies two or more protons (H+ ions) during an acid–base reaction
Polyprotic Acid
112
Includes both diprotic and triprotic acids
Polyprotic Acid
113
Transfers ~100% of its protons to water in an
aqueous solution
Equilibrium position lies far to the right
Strong Acid
114
Transfers only a small percent of its protons to water in an aqueous solution
Equilibrium position lies far to the left
Weak Acid
115
Hydroxides of Groups IA and IIA
Strong bases
116
An equilibrium constant for the reaction of a weak
acid with water
Acid Ionization Constant
117
Acid strength increases along with an increase in
______
Acid strength increases with an increase in the
______
Percent ionization increases with an increase in the
______
percent ionization, magnitude of Ka, magnitude of Ka
118
The stronger the acid, the ______ the Ka.
larger
119
The stronger the acid, the ______ the pKa.
smaller
120
The equilibrium constant for the reaction of a weak
base with water
Base Ionization Constant
121
The ______ indicates the concentration of protons is a solution.
pH
122
pH values decrease as the acidity of the solution
______.
increases
123
Solutions with pH values less than 7 are ______,
whereas those with pH values greater than 7 are
______.
acidic, basic
124
A Measure of Acidity
pH
125
pH = ______
-log [H+]
126
Ionic compounds containing a metal or polyatomic
ion as the positive ion and a nonmetal or polyatomic
ion (except hydroxide) as the negative ion
Salts
127
All common soluble salts are completely ______
into ions in solution
dissociated
128
The chemical reaction between an acid and a
hydroxide base in which a salt and water are the
products
Neutralization Reaction
129
In a neutralization reaction, what products are
formed?
Water and salt
130
The Henderson–Hasselbalch Equation
pKa = pH + log [HA]/[A–]
131
The ______ tells us whether (at a given pH) a compound will be in its acidic form (with its proton) or in is basic form (without its proton).
Henderson–Hasselbalch equation
