Chapter 2-3 Quiz (poly atomics) Flashcards
1
Q
Charge of Protons
A
Positive
1
Q
What charge do electrons have?
A
Negative?
1
Q
What is an atomic element?
A
A element that is usually found by itsself in nature.
1
Q
What is the charge of Scandium?
A
3+
1
Q
Hydrogen Sulfate or BI
A
HSO4(-)
2
Q
Cyanide
A
CN-
3
Q
Which types compounds get prefixes
A
Covalent
3
Q
CO3(2-)
A
Carbonate
3
Q
Hydrogen Phosphate or BI
A
HPO4(2-)
4
Q
What defines the element?
A
The number of protons
4
Q
What was Milikan’s contribution?
A
Used gravitational forces to suspend oil droplets and discovered that electrons had negative charge.
4
Q
Acid form of hydroxide
A
Hydrogen peroxide
4
Q
NH3
A
Acid form of ammonium
5
Q
What charges can tin have?
A
II or IV
5
Q
SO3(2-)
A
Sulfite
5
Q
HPO3(2-)
A
Hydrogen Phosphite
5
Q
Iodate
A
IO3(-)
6
Q
C2H302(-)
A
Acetate
7
Q
What types of elements form ionic bonds?
A
Metals and non Metals
8
Q
Cr2O7(2-)
A
DiChromate
9
Q
In which type of bond are electrons transferred?
A
Ionic
9
Q
What charges can nickel have?
A
II and IV
9
Q
ClO(-)
A
Hypochlorite
10
Q
What is a Molecular Element>?
A
An element that is found in a molecule with other atoms of its same kind in nature.
10
What charges can Chromium have?
II or III
10
Acid form of chromate
H2CrO4 Chromic acid
12
Naming Prefixes: 1: 2: 3: 4: 5: 6: 7: 8: 9: 10:
mono di tri tetra penta hexa hepta octa nona deca
12
HPO4(2-)
Hydrogen Phosphate or BI
13
What type of elements for covalent bonds?
Non metals and other non metals.
14
Chlorite
ClO2(-)
14
Phosphate
PO4(3-)
14
Ammonium
NH4(+)
15
What charges can Mercury have?
I or II
16
Sulfate
SO4(2-)
18
H2PO4(-)
Dihydrogen Phosphate
20
HSO3(-)
Hydrogen Sulfite or BI
21
HSO4(-)
Hydrogen Sulfate or BI
23
What is a structural formula?
A graphical representation of what a molecule looks like.
23
Carbonate
CO3(2-)
24
IO3(-)
Iodate
25
Chromate
CrO4(2-)
26
Permanganate
MnO4-
28
Bromate
BrO3(-)
29
02(2-)
Peroxide
30
Hydrogen Carbonate or BiCarbonate
HCO3(-)
31
How do you calculate atomic mass?
Weighted Averages
33
Hydrogen Sulfite or BI
HSO3(-)
34
What charges can copper have?
I or II
35
What is an ion
A negatively or positively charged particle
37
Hydronium
H30+
39
Acid form of cyanice
HCN Hydrocyanic Acid
40
What was Cadwicks's contribution?
Discovered the neutron, and that it had extra mass proportional to its charge.
40
Base form of Hydronioum
Water
42
HMnO4(-) Permanganic Acid
Acid form of permanganate
43
DiChromate
Cr2O7(2-)
44
What charges can lead have?
II or IV
45
Acetate
C2H302(-)
46
ClO2(-)
Chlorite
47
Whatis an acid?
Covalent bonded compounds that when disolved in water, hydrogens leave
47
Water
Base form of Hydronioum
48
What are the Molecular Elements?
Br2, I2, N2, Cl2, H2, O2, F2, P4, S8
49
What was Proust's contributions?
Law of definite proportions: all samples of a given compound have the same ratio.
50
CrO4(2-)
Chromate
52
Sulfite
SO3(2-)
53
DO protons add to atomic weight?
Yes
55
Which sub atomic particles have mass and which do not.
Electrons have negligible mass, protons and neutrons have mass.
56
What is molar mass?
Mass in grams of 1 mol of its molecules or formula units is numerically equivalent to its formula mass
57
HC2H3O2 Acetic Acid
Acid form of acetate (formula and name)
58
Hydrogen peroxide
Acid form of hydroxide
60
What was John Dalton's impact on chemisrty
Law of multiple proportions, Elements had definite ratios. 5 Main Points: 1. Elements come from atoms 2. Atoms of a given element are identical in size 3. Atoms cannot be created / destroyed 4. Atoms of different elements can combine in simple whole number ratios to form compounds. 5. In chemical reactions, atoms are combined, separated or rearranged.
61
How to name binary acids?
Hydro + element + ic + acid
63
What charges can iron have?
II or III
64
PO3(3-)
Phosphite
65
What is the charge of Silver
+
67
SO4(2-)
Sulfate
68
NH4(+)
Ammonium
69
What is another name for a covalent bond?
Molecular bond
70
PO4(3-)
Phosphate
71
HPO3(2-)
Hydrogen Phosphite or BI
72
Perchlorate
ClO4(-)
74
What is formula Mass?
Mass of an individual Molecule or Formula
75
What is one mol in units
6.022 \* 10^23
77
NO2-
Nitrite
78
What charges can manganese have?
II or III
79
CN-
Cyanide
81
What was Thompson's Contribution
Discovery of the electron, plum pudding model
82
What are Ionic Bonds held together by?
Oppisite charges between atoms.
83
What charge does a cation have
Positive
84
What is a hydrate?
Ionic compounds containing a specific number of water molecules associated with each formula unit
85
What is a oxyacid
Hydrogen and a polyatomic ion
87
Nitrate
NO3(-)
89
What are binary acids?
Hydrogen and one other element
90
Acid form of acetate (formula and name)
HC2H3O2 Acetic Acid
91
Dihydrogen Phosphite
H2PO3(-)
92
MnO4-
Permanganate
93
ClO3(-)
Chlorate
94
Hydrogen Phosphite or BI
HPO3(2-)
95
Dihydrogen Phosphate
H2PO4(-)
96
Chlorate
ClO3(-)
97
What charges can titanium have?
III and IV
98
What was Rutherford's contribution to chemistry
The discovery of a nucleus through the gold foil experiment.
99
Peroxide
02(-)
100
What was Medley's Contribtution
Organized the elements into a crude version of the periodic table.
101
How to name oxy acid
Polyatomic name + ic for ate OR ous for ite
102
H30+
Hydronium
103
Who was the father of chemistry
Lavoiser
103
What are covalent bonds held together by?
Shared electrons
104
Phosphite
PO3(3-)
107
What do we call covalent compounds?
Molecules
108
HCO3(-)
Hydrogen Carbonate or BiCarbonate
109
What charges can cobalt have?
II or III
111
ClO4(-)
Perchlorate
112
Chlorite
ClO2(-)
113
Nitrite
NO2-
114
What theory/ law did Lavoiser come up with?
Law of Conservation of Mass through the Theory of Combustion.
115
NO3(-)
Nitrate
116
What is the charge of Zinc?
2+
117
Acid form of permanganate
HMnO4 Permanganic Acid
118
Base form of ammonium
NH3
119
What charge do neutrons have?
Neutral
121
What is an empirical formula?
Lowest whole number ratio of atoms in a compound.
122
What is a molecular formula?
The actual number of atoms in a molecule of a substance.
123
What charge does a anion have
Negative
124
BrO3(-)
Bromate
