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Chemistry 101 > Unit 2 > Flashcards

Unit 2 Flashcards

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1
Q

pure substances

A

ionic and moleculer

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2
Q

composed of two or more different atoms which have chemically combined

A

ionic and molecular

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3
Q

whole number ratios of atoms (represented by chemical formula)

A

ionic and molecular

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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

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5
Q

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

A

molecular

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6
Q

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

A

ionic

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7
Q

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

A

molecular

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8
Q

notice: no metals, ions or charges

A

molecular

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9
Q

when we write ions by themselves we must indicate the charge

A

ionic

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10
Q

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

A

ionic compound

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11
Q

7 diatomic elements

A 
Hydrogen
Nitrogen
Oxygen
Fluorine
Chlorine
Bromine
Iodine
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12
Q

the second energy level contains how many sublevels

A

two

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13
Q

the first energy level contains how many sublevels

A

one

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14
Q

the fourth energy level contains how many sub levels

A

four

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15
Q

the fifth energy level contains how many sub levels

A

five

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16
Q

the third energy level contains how many sub levels

A

three

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17
Q

a P sublevel has how many orbitals

A

three

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18
Q

P sublevel has a maximum capacity of how many electrons

A

six

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19
Q

a S sublevel has how many orbitals

A

one

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20
Q

S sublevel has a maximum capacity of how many electrons

A

two

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21
Q

a F sublevel has how many orbitals

A

seven

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22
Q

F sublevel has a maximum capacity of how many electrons

A

14

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23
Q

D sublevel has how many orbitals

A

five

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24
Q

D sublevel has a maximum capacity of how many electrons

A

10

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25
Q

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

A

32

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26
Q

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

A

50

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27
Q

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

A

18

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28
Q

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

A

8

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29
Q

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

A

2

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30
Q

how many orbitals are present in the 3rd energy level

A

9

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31
Q

how many orbitals are present in the 1st energy level

A

1

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32
Q

how many orbitals are present in the 2nd energy level

A

4

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33
Q

5th energy level contains how many orbitals

A

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

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34
Q

4th energy level contains how many orbitals

A

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

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35
Q

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

A

8

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36
Q

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

A

2

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37
Q

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

A

2

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38
Q

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

A

2

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39
Q

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

A

8

40
Q

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

A

orbital

41
Q

approx mass of protons

A

1 amu

42
Q

approx mass of neutrons

A

1 amu

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

A

r=n2a0

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

A

bohr

50
Q

helped to explain emission spectra

A

bohr

51
Q

e- moves very fast and behaves like light

A

quantum mechanical model

52
Q

when it loses an electron it becomes

A

a cation

53
Q

when it gains an electron it becomes

A

an anion

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

A

true

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

A

(n-1)

64
Q

mL in quantum numbers represents

A

orbital

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

A

bohr

80
Q

who said there were energy levels

A

bohr

81
Q

maximum number of electrons= 2n^2

A

bohr

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

A

spherical

96
Q

p orbitals are

A

figure 8

97
Q

d orbitals are

A

4 clover leaf, 5th looks like double sided pacifier

Chemistry 101 (8 decks)

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