Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry 101 > Unit 2 > Flashcards

Unit 2 Flashcards

1
Q

pure substances

A

ionic and moleculer

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

composed of two or more different atoms which have chemically combined

A

ionic and molecular

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

whole number ratios of atoms (represented by chemical formula)

A

ionic and molecular

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

when elements chemically combine electrons are lost by the metals to form cations and electrons are gained by the nonmetals to form anions

A

ionic compounds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

when electrons chemically combine electrons are shared between atoms of nonmetals and/or metalloids

A

molecular

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

ions are not connected together to form a single unit. ions are held together by the attraction of opposite charges

A

ionic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

atoms are connected together by the shared electrons to form a larger unit called a molecule

A

molecular

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

notice: no metals, ions or charges

A

molecular

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

when we write ions by themselves we must indicate the charge

A

ionic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

amount of positive charge must balance the amount of negative charge in an ionic compound

A

ionic compound

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

7 diatomic elements

A 
Hydrogen
Nitrogen
Oxygen
Fluorine
Chlorine
Bromine
Iodine
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

the second energy level contains how many sublevels

A

two

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

the first energy level contains how many sublevels

A

one

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

the fourth energy level contains how many sub levels

A

four

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

the fifth energy level contains how many sub levels

A

five

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

the third energy level contains how many sub levels

A

three

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

a P sublevel has how many orbitals

A

three

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

P sublevel has a maximum capacity of how many electrons

A

six

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

a S sublevel has how many orbitals

A

one

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

S sublevel has a maximum capacity of how many electrons

A

two

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

a F sublevel has how many orbitals

A

seven

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

F sublevel has a maximum capacity of how many electrons

A

14

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

D sublevel has how many orbitals

A

five

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

D sublevel has a maximum capacity of how many electrons

A

10

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

4th energy level would contain how many electrons when completely filled

A

32

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

5th energy level would contain how many electrons when completely filled

A

50

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

3RD energy level would contain how many electrons when completely filled

A

18

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

2ND energy level would contain how many electrons when completely filled

A

8

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

1ST energy level would contain how many electrons when completely filled

A

2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

how many orbitals are present in the 3rd energy level

A

9

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

how many orbitals are present in the 1st energy level

A

1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

how many orbitals are present in the 2nd energy level

A

4

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

5th energy level contains how many orbitals

A

(# of energy level squared) 5^2= 25

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

4th energy level contains how many orbitals

A

(# of energy level squared) 4^2=16

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

the maximum number of electrons that can be found in the highest energy level of any atom is

A

8

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

maximum number of electrons that can be found in a single D orbital is

A

2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

maximum number of electrons that can be found in a single S orbital is

A

2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
38
Q

maximum number of electrons that can be found in a single P orbital is

A

2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
39
Q

those elements whose atoms have a stable electron configuration are members of group

40
Q

the volume in space where we are most likely to find an electron is an

41
Q

approx mass of protons

42
Q

approx mass of neutrons

43
Q

approx mass of electrons

A
  • 1/1830 amu
44
Q

what is the formula formed by Bohr for the radius of an electron

45
Q

how many electrons in the 4th energy level

A

32e- (2n^2)

46
Q

how many electrons in the 2nd energy level

A

8e- (2n^2)

47
Q

how many electrons in the 3rd energy level

A

18e- (2n^2)

48
Q

how many electrons in the 1st energy level

A

2e- (2n^2)

49
Q

viewed e- as slow moving particle moving around the nucleus

50
Q

helped to explain emission spectra

51
Q

e- moves very fast and behaves like light

A

quantum mechanical model

52
Q

when it loses an electron it becomes

53
Q

when it gains an electron it becomes

54
Q

a region in space where we are most likely to find an electron

A

quantum mechanical model

55
Q

e- in the outermost energy level

A

valence electrons

56
Q

e- that are not in the outermost energy level

A

core electrons

57
Q

known for their lack of reactivity

A

noble gases

58
Q

T or F noble gases are stable. they have nothing to gain by reacting

59
Q

all atoms want 8 valence electrons

A

octet rule

60
Q

all atoms want 8 valence electrons except

A

Helium (2 valence e-)

61
Q

n in quantum numbers represents

A

the energy level

62
Q

L in quantum numbers represents

A

the sub level

63
Q

equation for finding L

64
Q

mL in quantum numbers represents

65
Q

Ms in quantum numbers represents

A

electrons (arrows)

66
Q

no two electrons in an atom can have the same set of quantum numbers

A

pauli exclusion principle

67
Q

in orbital box diagrams each individual box represents WHAT and the entire ensemble represents WHAT

A

ORBITALS; SUBLEVEL

68
Q

each orbital of a sublevel must contain an electron before pairing can begin

A

hund’s rule

69
Q

how atoms interact to form molecules and compounds

A

chemical bonding

70
Q

write the symbol for the atom and then put dots around it to represent the number of valence electrons

A

lewis dot symbols

71
Q

transfer of one (or more) e- from a metal to a nonmetal to form cations and anions with noble gas electron configuration

A

ionic bonding

72
Q

pair of e- shared between two atoms

A

covalent bonding

73
Q

using a diffraction grating plus a source of white light, we see a

A

continuous spectrum

74
Q

all energies of light are being emitted

A

continuous spectrum

75
Q

using a diffraction grating and a sample of Hydrogen with high voltage electricity is passed, we see

A

line spectrum

76
Q

only a few energies of light are emitted

A

line spectrum

77
Q

Each element has it’s own unique

A

line spectrum

78
Q

only way to separate a covalent bond is a

A

chemical change

79
Q

who said that electrons in orbit

80
Q

who said there were energy levels

81
Q

maximum number of electrons= 2n^2

82
Q

sublevels - s,p,d,f,g,h,i

A

quantum mechanical model

83
Q

sublevels composed of orbitals

A

quantum mechanical model

84
Q

energies of a sub level (or order of filling)

A

Aufbau principle

85
Q

three methods of writing - spectroscopic notation, orbital box diagrams, quantum numbers

A

electron configuration

86
Q

electron(s) are transferred from metal to nonmetal

A

Ionic Bonding

87
Q

ions are not attached to one another

A

Ionic Bonding

88
Q

full charges

A

Ionic Bonding

89
Q

ionic bond – the force of attraction between oppositely charged ions

A

Ionic Bonding

90
Q

sharing electrons – two nonmetals or metalloid & nonmetal

A

Covalent Bonding

91
Q

atoms are connected by covalent bond – molecule

A

Covalent Bonding

92
Q

Seven diatomic elements

A

Covalent Bonding

93
Q

metal and nonmetal

A

ionic bond

94
Q

two nonmetals

A

covalent bond

95
Q

s orbitals are

96
Q

p orbitals are

97
Q

d orbitals are

A

4 clover leaf, 5th looks like double sided pacifier

Chemistry 101 (8 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions