exam 2 Flashcards
(105 cards)
1
Q
Electrons are described as likely to be found in a specific region of a space called an orbital
A
Quantum Model
2
Q
Principal quantum number, number, n, row number from the periodic table
A
Energy Level/Shell
3
Q
s, p, d, or f type, each has a set number of possible orbitals
A
Sublevel/Subshell
4
Q
Probability map for locating an electron of a certain energy
- Each type has a specific shape in 3D
- Can hold up to 2 electrons (of opposite spin)
A
Orbital
5
Q
The electrons in the highest principal energy level (whole level, largest n value)
A
Valence Electrons
6
Q
8 electrons in the valence level, atoms tend to react chemically to attain an octet of electrons in the valence level (ns^2np^6)
A
Octet Rule
7
Q
Sharing valence level electrons to achieve access to an octet
A
Covalent Bonding
8
Q
How many covalent bonds does hydrogen form?
A
1
9
Q
How many covalent bonds does Group 3A/13 form?
A
3
10
Q
How many covalent bonds does Group 4A/14 form?
A
4
11
Q
How many covalent bonds does Group 5A/15 form?
A
3
12
Q
How many covalent bonds does Group 6A/16 form?
A
2
13
Q
How many covalent bonds does Group 7A/17 form?
A
1
14
Q
How many covalent bonds does Group 8A/18 form?
A
Does not form covalent bonds
15
Q
What is the ionic charge of Group 1A/1?
A
1+
16
Q
What is the ionic charge of Group 2A/2?
A
2+
17
Q
What is the ionic charge of Al?
A
3+
18
Q
What is the ionic charge of Ag?
A
1+
19
Q
What is the ionic charge of Zn?
A
2+
20
Q
What is the ionic charge for Group 3A/13?
A
0
21
Q
What is the ionic charge for Group 4A/14?
A
4+
22
Q
What is the ionic charge for Group 5A/15?
A
3-
23
Q
What is the ionic charge for Group 6A/16?
A
2-
24
Q
What is the ionic charge for Group 7A/17?
A
1-
25
What is the ionic charge for Group 8A/18?
Does not form ions
26
Atoms transfer electrons (lose/gain) to form ions
Ionic Bond
27
1 pair of electrons shared between 2 atoms
Single Bond
28
2 pairs of electrons shared between 2 atoms
Double Bond
29
3 pairs of electrons shared between 2 atoms
Triple Bond
30
Shared pairs between 2 atoms
Bonding Pairs
31
Pairs unshared on an individual atom
Nonbonding/Lone Pairs
32
Made from 2 types of nonmetal atoms
Binary Molecular Compound
33
mono-
1
34
di-
2
35
tri-
3
36
tetra-
4
37
penta-
5
38
hexa-
6
39
Chemical bonding by electron transfer, between metals and nonmetals
Ionic Bonding
40
Chemical bonding by electron sharing, between different nonmetal atoms
Molecular/covalent Bonding
41
The smallest component of an element
Atom
42
A charged atom
Ion
43
A charged group of bonded atoms
Polyatomic Ion
44
6.022 x 10^23
Avogadro's Number also =1 mole
45
Represents the simplest whole ratio of atoms in a compound
Empirical Formula
46
Represents the true count of atoms in one molecule
| -Will be the same as or a whole number multiple of the empirical formula
Molecular Formula
47
- Tend to be brittle, crystalline
- Tend to be very high melting solids (usually solids at room temperature)
- Many are water soluble
- Act as electrolytes when molten or in water solution
Ionic Compounds
48
- Tend to be soft, powdery, or waxy solids
- Tend to have moderate melting points
- Many are gases or liquids at room temperature
- Some are water soluble and many are insoluble
- Usually non electrolytes when molten or in water solution
- Will form molecular crystals with individual molecules when interacting with each other
Molecular Compounds
49
Appears uniform in composition, is uniform in composition
Homogeneous
50
The component that has the greatest quantity, the dissolving agent
Solvent
51
The substance dissolved, all other components
Solute
52
Solution where water is the solvent
Aqueous
53
Able to be dissolved
Soluble
54
Incapable of being dissolved
Insoluble
55
Remain intact as whole molecules when dissolved in water
Polar molecular
56
Dissociated into ions when dissolved in water
Nonpolar molecular
57
"Like dissolves like"
| Lots of favorable solute-solvent interactions, solution forms
Polar-polar
58
"Like dissolves like"
| No solution
Polar-nonpolar
59
"Like dissolves like"
| Not much solvent-solute interaction, but solution forms
Nonpolar-nonpolar
60
Ionic compounds often do dissolve in ionizing solvent and water is one of the only known ionizing solvents, most ionics dissolve in water
Ionics-water
61
Conduct an electrical current when molten or in water solution
Electrolytes
62
Do not conduct an electrical current even when molten or in water solution
Nonelectrolytes
63
Conduct electricity well, many ions present
- Forms essentially all ions
- Water soluble ionic compounds
- Strong acids and bases
Strong Electrolytes
64
Do conduct, but not well, few ions present
- Weak acids and bases
- Barely soluble ionic compounds
Weak Electrolytes
65
Do not conduct an electrical current
- No ions present
- Most molecular substances remaining as whole molecules when dissolved in water
Nonelectrolytes
66
Study of compounds that contain carbon (will always contain hydrogen and carbon)
Organic Chemistry
67
What makes carbon special?
1. Forms up to 4 covalent bonds
2. Forms very strong covalent bonds
3. Forms multiple bonds (double and triple bonds, almost no other element does this)
4. Can combine to form very large arrays in rings, chains, and branched chains by C-C bonding, very unusual
68
Represents the bonding attachments of the atoms within the compound
Structural Compound
69
Represents the ratio of atoms within the compound
Molecular Formula
70
Different compounds that are related by having the same molecular formula
Isomers
71
Different momentary rotations of the same molecule
Conformers
72
A compound that contains only carbon and hydrogen
Hydrocarbon
73
Carbons linked consecutively in one line
Straight Chain
74
At least 1 carbon group hanging off the main chain
Branched Structure
75
A closed geometric shape that is made from at least some of the carbons
Ring/Cyclic Structure
76
A ring structure which contains an atom other than carbon as an integral (direct) part of the ring itself
Heterocyclic
77
An atom other than carbon or hydrogen in an organic compound
Heteroatom
78
Specific atom, or usually a cluster of atoms, responsible for creating properties and reactions of a specific type of atom
Functional Group
79
Single bonds between carbons, hydrocarbons only
Alkanes
80
At least 1 carbon to carbon double bond, hydrocarbons only
Alkenes
81
At least 1 carbon to carbon triple bond, hydrocarbons only
Alkynes
82
A 6-membered ring with alternating single and double carbon to carbon bonds, only hydrocarbons
Aromatic
83
A carbon single bonded to an oxygen single bonded to an hydrogen; C, H, O
Alcohol
84
An alcohol where the carbon with the OH on it is a direct part of an aromatic ring; C, H, O
Phenol
85
An oxygen single bonded to 2 carbons; C, H, O
Ether
86
A carbon double bonded to an oxygen with at least 1 of the remaining 2 bonds from carbon being a single bond to hydrogen; C, H, O
Aldehyde
87
A carbon double bonded to an oxygen with both of the remaining 2 bonds from carbon being single bonds to another carbon; C, H, O
Ketone
88
A carbon double bonded to an oxygen and that same carbon single bonded to another oxygen that is then single bonded to a carbon; C, H, O
Carboxylic Acid
89
A carbon double bonded to an oxygen and that same carbon is single bonded to an oxygen that is then single bonded to a carbon; C, H, O
Ester
90
A nitrogen that is single bonded to at least 1, and up to 3, carbons; C, H, N
Amine
91
A carbon that is double bonded to an oxygen and that same carbon is single bonded to a nitrogen; C, H, N
Amide
92
Polyhydroxyl aldehydes or ketones (many alcohols, ketones, aldehydes)
Simple Carbohydrates
93
Have both carboxylic acids and amino (amine) groups
Amino Acids
94
Amino acids that are linked together
Peptides
95
Polyamides (polypeptides)
Proteins
96
Long carboxylic acids--usually long chains of carbon
Fatty Acids
97
Triesters of the alcohol glycerol
Fats and Oils
98
Same side, as in both below or above
Cis
99
Opposite sides, as in one below and one above
Trans
100
An organic molecule that is carbon singly bonded (tetrahedral carbon) to 4 different atoms or clusters of atoms
Chiral Carbon
101
The amount of a specific product actually obtained from a reaction, an experimental measurement, what is collected
Actual Yield
102
Obtained from the balanced equation and a stoichiometry calculation; what is possible to get
Theoretical Yield
103
The proportion of the maximum possible yield and the actual obtained yield as a %
Percent Yield
104
May mean a poor technique was involved, may mean the reaction itself did not go to completion
Low % Yield
105
The reaction did go to completion and careful technique was used
High % Yield
