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? General Chemistry > 1. Atoms and Molecules > Flashcards

1. Atoms and Molecules Flashcards

(105 cards)

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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
what is group 3-12 known as
transition metals
26
group 1 elements form what charge of ions
1+ cations
27
what is group 2 known as
alkaline earth metals
28
group 2 elements form what charge of ions
2+ cations
29
group 2 elements have how many valence e-
2
30
group 1 elements have how many valence e-
1
31
what is group 14 known as alternately and how many covalent bonds can they form and with which types of elements
group 4 forms 4 covalent bonds with non metals
32
how many valence e- does group 14 elements have
4
33
how many covalent bonds can group 15 elements form
3 covalent bonds
34
how many valence e- does group 15 elements have
5
35
what group contains oxygen
16
36
what is group 17 known as
halogens
37
how reactive are group 17 and how many bonds can it form with other elements
very reactive forms one bond with other elements
38
what is group 18 known as and how reactive are they
noble gases nonreactive
39
how many valence e- does group 18 have
none, they have full outer shells
40
how does an element become an ion
when it has more or less e- than protons
41
what are negative ions known as
anions
42
what are positive ions known as
cations
43
what is the suffix of anions
-ide
44
as you move from left to right along the periodic table what happens to the atomic size, electronegativity and ionisation energy
atomic size decreases electronegativity and ionisation energy increases
45
as you move down the periodic table what happens to the atomic size, electronegativity and ionisation energy
atomic size increases electronegativity and ionisation energy decreases
46
why does atomic size/radius increase from right to left
effective nuclear charge increases (more protons) from left to right and each additional e- is pulled more strongly to the nucleus
47
why does atomic size/radius increase from top to bottom
atoms becomes larger with each added shell
48
when moving down the periodic table each underlying period will have elements with what changing in terms of e-
with an extra shell of e-
49
what is ionization energy
energy required to remove e- from atom
50
why is more energy required to be removed for some elements and thus have a higher ionisation energy
if an e- is more strongly attached to nucleus requires more energy to be removed
51
why does ionisation energy increase from left to right
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
why does ionisation increase when moving up the periodic table
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
what is electronegativity
tendency of atom to attract e- in a bond that it shares with another atom
54
what is a covalent bond
2 e- shared by 2 nuclei
55
what happens to the e- in a covalent bond
the 2 negatively charged e- are pulled toward both positively charged nuclei via electrostatic forces
56
what is a hydrogen bond
dipole forces attractive force between hydrogen attached to an electronegative atom of one molecule and an electronegative atom of a different molecule
57
what is the charge of the 2 atoms in the hydrogen bond
hydrogen has partial positive charge other atom has partial negative charge
58
what is an ionic bond
chemical bond involving electrostatic attraction between oppositely charged ions
59
what are van der waals interactions
interaction of e- clouds between molecules
60
what is the weakest intermolecular attraction
van der waals
61
is van der waals interactions intra/intermolecular
intermolecular
62
what are hydrophobic interactions
intermolecular interactions between non polar substances
63
what is an empirical formula
simplest whole number ratio between number of atoms of different elements in the compound
64
what is NH4+
ammonium
65
what is H3O+
hydronium
66
what is CH3COO-
acetate
67
what is CN
cyanide
68
what is OH-
hydroxide
69
what is ClO-
hypochlorite
70
what is ClO2-
chlorite
71
what is ClO3-
chlorate
72
what is ClO4-
perchlorate
73
what is NO2-
nitrite
74
what is NO3-
nitrate
75
what is MnO4-
permanganate
76
what is CO3 2-
carbonate
77
what is CrO4 2-
chromate
78
what is C2rO7 2-
dichromate
79
what is O2 2-
peroxide
80
what is PO4 3-
phosphate
81
what is SO3 2-
sulfide
82
what is SO4 2-
sulfate
83
what is the law of conservation of mass
number of atoms of a given element remains constant during a chemical reaction
84
what is a synthesis/combination reaction in terms of ABC
simple substances combine to give compound A + B -> AB
85
what is a decomposition reaction in terms of ABC
compound broken down into simpler substances AB -> A + B
86
what is a substitution/single displacement reaction in terms of ABCD
atom/group of atoms replaced by another atom/group of atoms A + BC -> B + AC or BA + C
87
what is a precipitation/double displacement reaction in terms of ABCD
solid compound formed when solutions of 2 soluble compounds are mixed AB + CD -> AD + BC
88
what is a neutralisation reaction in terms of ABC
acid reacts with base giving salt and water HA + BOH -> H2O + BA
89
what is a redox reaction
electron transfer occurs reduction = A -> A+ + e- oxidation = B+ + e- -> B
90
what does oxidised mean in terms of oxidation number
reaction if oxidation number increases
91
what does reduced mean in terms of oxidation number
oxidation number decreases
92
what is the oxidation number for an atom in elemental form what are the 2 conditions that means a substance is elemental
always 0 only one kind of atom is present if charge is 0
93
what is the oxidation number of a monoatomic ion
the charge of the monoatomic ion
94
what is the oxidation number of all group 1 metals
+1 unless elemental
95
what is the oxidation number of all group 2 metals
96
what is the oxidation number of all group 2 metals
2+ unless elemental
97
what is the oxidation number of hydrogen
+1 when bonded to nonmetal -1 when bonded to metal
98
what is the oxidation number of oxygen
-1 in peroxides (O2 2-) -2 in all other compounds
99
what is the oxidation number of fluorine
-1
100
what is the oxidation number of a neutral compound
sum of all oxidation numbers of all atoms/ions in neutral compound = 0
101
what is the oxidation number of a polyatomic ion
sum of all oxidation numbers of all atoms in polyatomic ion = charge on polyatomic ion
102
what is a oxidising agent in terms of what it causes to happen and what happens to the agent itself
will cause oxidation to occur agent itself will be reduced
103
what is a reducing agent in terms of what it causes to happen and what happens to the agent itself
causes reduction to occur agent itself will be oxidised
104
what is reduction in terms of e-
gain of e-
105
what is oxidation in terms of e-
loss of e-

? General Chemistry (7 decks)

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