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Chemistry > 1 semester test > Flashcards

1 semester test Flashcards

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1
Q

extensive property

A

changes with the amount

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2
Q

intensive property

A

does not change with the amount

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3
Q

6 signs of chemical change

A
  • color change
  • temperature change
  • odor
  • precipitate
  • light emitted
  • gas produced
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4
Q

magic 7 diatomic elements

A
  • H
  • N
  • O
  • F
  • Cl
  • Br
  • I
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5
Q

liquid to gas

A

evaporation

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6
Q

gas to solid

A

deposition

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7
Q

solid to liquid

A

melting

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8
Q

liquid to solid

A

freezing

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9
Q

solid to gas

A

sublimation

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10
Q

gas to liquid

A

condensation

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11
Q

what is accuracy

A

correctness

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12
Q

what is precision

A

reproducibility

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13
Q

percent error formula

A

%error=(actual-measured)/actualx100

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14
Q

1kg is how many grams

A

1000

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15
Q

1km is how many m

A

1000

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16
Q

100 cm is how many m

A

1

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17
Q

1000mm is how many m

A

1

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18
Q

1000mL is how many L

A

1

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19
Q

Dalton’s theory

A
  • all matter is composed of tiny indivisible particles called atoms (true)
  • all atoms of an element are identical (false)
  • atoms cannot be created, divided, or destroyed (false, atoms can be divided)
  • atoms of different elements combine chemically to form compounds(true)
  • atoms of 1 element cannot change into a new element during chemical reactions (true)
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20
Q

who experimented with the cathode ray tube

A

JJ Thompson

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21
Q

who used the gold foil experiement

A

Ernest Rutherford

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22
Q

who discovered the existence of neutrons

A

James Chadwick (jimmy neutron)

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23
Q

who proposed that electrons are arranged in 7 circular orbits

A

Niels Bohr

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24
Q

isotope notation

A

potassium-39 or 39
K
19

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25
Q

average atomic mass formula

A

(%abundance X mass #) + (%abundance X mass#)

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26
Q

how do cations form positive ions

A

lose electrons

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27
Q

how do anions form negative ions

A

gain electrons

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28
Q

what is an atom

A

single element

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29
Q

what is a molecule

A

compound of two or more non metals

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30
Q

what is a formula unit

A

compound with a metal bonded to non metal

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31
Q

how many electrons can an orbital hold

A

2 electrons

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32
Q

what is the ground state

A

most stable, lowest energy arrangement of the electrons in an atom

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33
Q

what is the excited state

A

atom gains energy and electrons jump into higher energy levels

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34
Q

ground to excited

A

absorb energy

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35
Q

excited to ground

A

release energy

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36
Q

representative element for atomic radii or ionic radii

A

Fr Francium

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37
Q

representative element ionization energy

A

He Helium

38
Q

representative element for electronegativity

A

F Fluorine

39
Q

what is a metallic bond

A

2 or more metals

40
Q

physical properties of metallic bonds

A

electrons are mobile = conduct electricity & heat
atoms are hard to pull apart bc of sea of e-
ductile and malleable

41
Q

ionic bonding

A

bonding between 2 ions (nm and m)

42
Q

what is the polyatomic symbol and charge for acetate

A

C2H3O2 -1

43
Q

what is the polyatomic symbol and charge for nitrite

A

NO2 -1

44
Q

what is the polyatomic symbol and charge for nitrate

A

NO3 -1

45
Q

what is the polyatomic symbol and charge for hydroxide

A

OH -1

46
Q

what is the polyatomic symbol and charge for carbonate

A

CO3 -2

47
Q

what is the polyatomic symbol and charge for sulfite

A

SO3 -2

48
Q

what is the polyatomic symbol and charge for sulfate

A

SO4 -2

49
Q

what is the polyatomic symbol and charge for phosphite

A

PO3 -3

50
Q

what is the polyatomic symbol and charge for phosphate

A

PO4 -3

51
Q

what is the polyatomic symbol and charge for ammonium

A

NH4 +1

52
Q

what is the polyatomic symbol and charge for hydronium

A

H3O +1

53
Q

covalent bonds are the result of the sharing of what

A

valence electrons

54
Q

linear molecular shapes have what bond angles

A

180

55
Q

trigonal planar molecular shapes have what bond angles

A

120

56
Q

tetrahedral molecular shapes have what bond angles

A

109.5

57
Q

trigonal pyramidal molecular shapes have what bond angles

A

107.3

58
Q

bent molecular shapes have what bond angles

A

104.5

59
Q

what is an alloy

A

mixture of 2 or more metals

60
Q

what is the strongest bond

A

ionic

61
Q

what bond has the highest melting point

A

ionic

62
Q

what bond has the lowest melting point

A

covalent

63
Q

what is the weakest bond

A

covalent

64
Q

what is the strongest bond

A

ionic

65
Q

mono

A

1

66
Q

di

A

2

67
Q

tri

A

3

68
Q

tetra

A

4

69
Q

penta

A

5

70
Q

hexa

A

6

71
Q

hepta

A

7

72
Q

octa

A

8

73
Q

nona

A

9

74
Q

deca

A

10

75
Q

nitrogen trihydride NH3 is what

A

ammonia

76
Q

carbon tetrahydride CH4 is what

A

methane

77
Q

no “O” means to

A

use prefix “hydro” Hydro___ic acid

78
Q

with “O” means to

A

not use “hydro”

79
Q

ate to

A

ic

80
Q

ite to

A

ous

81
Q

moles flow chart

A

grams moles particles (funs to ions, atoms, molecules to atoms)

82
Q

what is empirical formula

A

simplest whole # (reduced)

83
Q

what is molecular formula

A

the real formula (not reduced)

84
Q

4 steps to writing empirical formula

A
  1. determine number of grams for each element (% to g)
  2. turn grams into moles for each element
  3. divide by smallest mole # (keep 4 decimals)
  4. if not all whole numbers, multiply to get whole #
85
Q

molecular formula

A

molecular mass of compound/empirical mass of compound (real/reduced)

86
Q

In the formula C=λν, what is the value of the C constant

A

speed of light 3x10^8

87
Q

in the formula E=hν, what is the value of the h constant

A

planck’s constant 6.63x10^-34

88
Q

for polarity, 0.3 and below is

A

non polar

89
Q

for polarity, 0.3 to 1.7 is

A

covalent

90
Q

for polarity, 1.7 and above is

A

ionic

Chemistry (5 decks)

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