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? General Chemistry > 1. Atoms and Molecules > Flashcards

1. Atoms and Molecules Flashcards

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1
Q

what is each atom composed of

A

nucleus surrounded by e- cloud

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2
Q

what composes a nucleus

A

protons and neutrons

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3
Q

what is the charge of e- and protons in terms of magnitude

A

opposite charges of equal magnitudes

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4
Q

what is the size comparison between protons, neutrons and e-

A

proton and neutron approx equal size but e- is much smaller

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5
Q

what is an element and what does it contain

A

chemical substance containing atoms that have same # of protons in atomic nuclei

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6
Q

what is the mass number

A

number of protons + neutrons in nucleus

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7
Q

what is the atomic number

A

number of protons in nucleus

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8
Q

what is the element characterised by

A

number of protons

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9
Q

if the proton, neutrons or e- # change will it still be the same element

A

protons = no

neutron and e- = yes

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10
Q

what are isotopes

A

2 atoms of same element that have diff mass # (different # of neutrons)

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11
Q

what is the atomic weight or molar mass of an atom and what is it measured in

A

atomic mass units (amu) is a ratio and defined by C12

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12
Q

what is the amu of C12

A

12amu

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13
Q

what is a mole

A

number of carbond atoms in 12 grams of C12

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14
Q

what is avogadros number and what does it define

A

defines number of C atoms in 12 grams of C as 6.022 x 10^23

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15
Q

what is avogadros number and what does it define

A

defines number of C atoms in 12 grams of C as 6.022 x 10^23

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16
Q

what is the formula relating moles, mass and molar mass together

A

n (moles) = m (mass in grams)/M (molar mass)

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17
Q

what is a vertical column in the periodic table called

A

group/family

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18
Q

what is a horizontal row in the periodic table called

A

period/row

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19
Q

what is the relative melting point and ion formation trend of non metals compared to metals

A

lower mp and form - ions

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20
Q

what happens to the e- in positive ion formation

A

lost e-

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21
Q

all positive ions are metals except for which 2

A

H+

NH4+

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22
Q

what happens to the e- in negative ion formation

A

gained e-

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23
Q

molecular substances are usually made up of what

A

only non metals

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24
Q

what is group 1 known as

A

alkali metals

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25
Q

what is group 3-12 known as

A

transition metals

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26
Q

group 1 elements form what charge of ions

A

1+ cations

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27
Q

what is group 2 known as

A

alkaline earth metals

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28
Q

group 2 elements form what charge of ions

A

2+ cations

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29
Q

group 2 elements have how many valence e-

A

2

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30
Q

group 1 elements have how many valence e-

A

1

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31
Q

what is group 14 known as alternately and how many covalent bonds can they form and with which types of elements

A

group 4 forms 4 covalent bonds with non metals

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32
Q

how many valence e- does group 14 elements have

A

4

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33
Q

how many covalent bonds can group 15 elements form

A

3 covalent bonds

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34
Q

how many valence e- does group 15 elements have

A

5

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35
Q

what group contains oxygen

A

16

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36
Q

what is group 17 known as

A

halogens

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37
Q

how reactive are group 17 and how many bonds can it form with other elements

A

very reactive

forms one bond with other elements

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38
Q

what is group 18 known as and how reactive are they

A

noble gases

nonreactive

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39
Q

how many valence e- does group 18 have

A

none, they have full outer shells

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40
Q

how does an element become an ion

A

when it has more or less e- than protons

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41
Q

what are negative ions known as

A

anions

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42
Q

what are positive ions known as

A

cations

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43
Q

what is the suffix of anions

A

-ide

44
Q

as you move from left to right along the periodic table what happens to the atomic size, electronegativity and ionisation energy

A

atomic size decreases

electronegativity and ionisation energy increases

45
Q

as you move down the periodic table what happens to the atomic size, electronegativity and ionisation energy

A

atomic size increases

electronegativity and ionisation energy decreases

46
Q

why does atomic size/radius increase from right to left

A

effective nuclear charge increases (more protons) from left to right and each additional e- is pulled more strongly to the nucleus

47
Q

why does atomic size/radius increase from top to bottom

A

atoms becomes larger with each added shell

48
Q

when moving down the periodic table each underlying period will have elements with what changing in terms of e-

A

with an extra shell of e-

49
Q

what is ionization energy

A

energy required to remove e- from atom

50
Q

why is more energy required to be removed for some elements and thus have a higher ionisation energy

A

if an e- is more strongly attached to nucleus requires more energy to be removed

51
Q

why does ionisation energy increase from left to right

A

greater nuclear charge (more protons) from left to right so more protons to create stronger attraction with surrounding e- so more ionisation energy required to remove e- from atom

52
Q

why does ionisation increase when moving up the periodic table

A

distance of e- from nucleus decreases moving up the table as there are less e- shells going up the table

decreased distance creates an increase in electric field strength and more energy is required to remove an e-

53
Q

what is electronegativity

A

tendency of atom to attract e- in a bond that it shares with another atom

54
Q

what is a covalent bond

A

2 e- shared by 2 nuclei

55
Q

what happens to the e- in a covalent bond

A

the 2 negatively charged e- are pulled toward both positively charged nuclei via electrostatic forces

56
Q

what is a hydrogen bond

A

dipole forces

attractive force between hydrogen attached to an electronegative atom of one molecule and an electronegative atom of a different molecule

57
Q

what is the charge of the 2 atoms in the hydrogen bond

A

hydrogen has partial positive charge

other atom has partial negative charge

58
Q

what is an ionic bond

A

chemical bond involving electrostatic attraction between oppositely charged ions

59
Q

what are van der waals interactions

A

interaction of e- clouds between molecules

60
Q

what is the weakest intermolecular attraction

A

van der waals

61
Q

is van der waals interactions intra/intermolecular

A

intermolecular

62
Q

what are hydrophobic interactions

A

intermolecular interactions between non polar substances

63
Q

what is an empirical formula

A

simplest whole number ratio between number of atoms of different elements in the compound

64
Q

what is NH4+

A

ammonium

65
Q

what is H3O+

A

hydronium

66
Q

what is CH3COO-

A

acetate

67
Q

what is CN

A

cyanide

68
Q

what is OH-

A

hydroxide

69
Q

what is ClO-

A

hypochlorite

70
Q

what is ClO2-

A

chlorite

71
Q

what is ClO3-

A

chlorate

72
Q

what is ClO4-

A

perchlorate

73
Q

what is NO2-

A

nitrite

74
Q

what is NO3-

A

nitrate

75
Q

what is MnO4-

A

permanganate

76
Q

what is CO3 2-

A

carbonate

77
Q

what is CrO4 2-

A

chromate

78
Q

what is C2rO7 2-

A

dichromate

79
Q

what is O2 2-

A

peroxide

80
Q

what is PO4 3-

A

phosphate

81
Q

what is SO3 2-

A

sulfide

82
Q

what is SO4 2-

A

sulfate

83
Q

what is the law of conservation of mass

A

number of atoms of a given element remains constant during a chemical reaction

84
Q

what is a synthesis/combination reaction in terms of ABC

A

simple substances combine to give compound

A + B -> AB

85
Q

what is a decomposition reaction in terms of ABC

A

compound broken down into simpler substances

AB -> A + B

86
Q

what is a substitution/single displacement reaction in terms of ABCD

A

atom/group of atoms replaced by another atom/group of atoms

A + BC -> B + AC or BA + C

87
Q

what is a precipitation/double displacement reaction in terms of ABCD

A

solid compound formed when solutions of 2 soluble compounds are mixed

AB + CD -> AD + BC

88
Q

what is a neutralisation reaction in terms of ABC

A

acid reacts with base giving salt and water

HA + BOH -> H2O + BA

89
Q

what is a redox reaction

A

electron transfer occurs

reduction = A -> A+ + e-
oxidation = B+ + e- -> B

90
Q

what does oxidised mean in terms of oxidation number

A

reaction if oxidation number increases

91
Q

what does reduced mean in terms of oxidation number

A

oxidation number decreases

92
Q

what is the oxidation number for an atom in elemental form

what are the 2 conditions that means a substance is elemental

A

always 0

only one kind of atom is present
if charge is 0

93
Q

what is the oxidation number of a monoatomic ion

A

the charge of the monoatomic ion

94
Q

what is the oxidation number of all group 1 metals

A

+1

unless elemental

95
Q

what is the oxidation number of all group 2 metals

A
96
Q

what is the oxidation number of all group 2 metals

A

2+

unless elemental

97
Q

what is the oxidation number of hydrogen

A

+1 when bonded to nonmetal
-1 when bonded to metal

98
Q

what is the oxidation number of oxygen

A

-1 in peroxides (O2 2-)

-2 in all other compounds

99
Q

what is the oxidation number of fluorine

A

-1

100
Q

what is the oxidation number of a neutral compound

A

sum of all oxidation numbers of all atoms/ions in neutral compound = 0

101
Q

what is the oxidation number of a polyatomic ion

A

sum of all oxidation numbers of all atoms in polyatomic ion = charge on polyatomic ion

102
Q

what is a oxidising agent in terms of what it causes to happen and what happens to the agent itself

A

will cause oxidation to occur

agent itself will be reduced

103
Q

what is a reducing agent in terms of what it causes to happen and what happens to the agent itself

A

causes reduction to occur

agent itself will be oxidised

104
Q

what is reduction in terms of e-

A

gain of e-

105
Q

what is oxidation in terms of e-

A

loss of e-

? General Chemistry (7 decks)

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