Test 1 Chemistry 116 Flashcards
(152 cards)
1
Q
Matter
A
A substance that has mass and occupies space
2
Q
States of Matter
A
Solid, liquid, gas
3
Q
Mixture (homogenous, heterogeneous)
A
Matter containing more than one type of atom, molecule, etc.
Homogenous: uniform consistency
Heterogenous: non-uniform consistency
4
Q
Scientific Method
A
- Question
- Research
- Hypothesis
- Experiment
- Data Analysis
- Conclusion
- Communication
5
Q
Theory v.s. Law
A
Theory: Tested, unifying statement explaining a series of observations
Law: Conceptual or mathematical statement about what is observed in nature (fact)
6
Q
Accuracy v.s. Precision
A
Accuracy: how close results how to a known
Precision: how close results are to each other
7
Q
Sig Fig +/- Rule
A
Answer has the amount of decimal points as the number with the fewest decimal places
8
Q
Sig Fig x/div Rule
A
Answer has the amount of sig figs as the number with the fewest sig figs
9
Q
SI Units for mass, length, volume, and temperature
A
kg, m, m^3 (L), kelvin
10
Q
Fahrenheit Formula
A
F= (9/5 C) +32
11
Q
Celsius Formula
A
C= (5/9)(F - 32)
12
Q
Kelvin Formula
A
K= C+273.15
13
Q
SI Prefix- Mega (M)
A
10^6 from m
14
Q
SI Prefix- Kilo (k)
A
10^3 from m
15
Q
SI Prefix- Deci (d)
A
10^-1 from m
16
Q
SI Prefix- Centi (c)
A
10^-2 from m
17
Q
SI Prefix- Milli (m)
A
10^-3 from m
18
Q
SI Prefix- Micro (u)
A
10^-6 from m
19
Q
SI Prefix- Nano (n)
A
10^-9 from m
20
Q
SI Prefix- Pico (p)
A
10^-12 from m
21
Q
Solids have a ___ shape and are not appreciable ___
A
definite, compressible
22
Q
If matter is uniform throughout, cannot be separated by physical processes but can be decomposed into other substances by chemical processes, it’s called___
A
Compound
23
Q
Initial tentative explanation of an observation
A
Hypothesis
24
Q
One degree of temperature difference is smallest on the __ scale.
A
Fahrenheit
25
Freezing point at
C-
F-
K-
0, 32, 273.15
26
Dalton's Postulates
1. Elements are composed of small particles known as atoms
2. All atoms of given element are identical to one another in mass and other properties (and vice versa)
3. Atoms of an element cannot change into atoms of another element
4. Compounds are formed when atoms of more than one element combine
27
Law of Conservation of Matter
The mass of the products= mass of the reactants
Matter is neither created or destroyed (minus nuke reactions)
28
Law of Multiple Proportions
When elements combine, they do so in a ratio of small whole numbers
29
Who discovered the Law of Multiple Proportions
Dalton
30
31
32
Matter
Any substance that has mass and occupies space
33
Atoms
The fundamental building blocks of matter
34
Types of Mixtures
Homogenous: uniform comp. ex: saltwater, sugar water
Heterogenous: non-uniform
35
Types of Pure Substances
Compound: can be chemically decomposed
Element: can't be chemical decomposed
36
Initial/tentative explanation of an observation
Hypothesis
37
SI units for mass, length, volume, temperature
kg, m, m^3 (L), Kelvin
38
Celsius Equation
C= (5/9)(F-32)
39
Fahrenheit Equation
F= (9/5C)+32
40
Kelvin Equation
K= C+273.15
41
SI Prefix - Mega
10^6
42
SI Prefix - Kilo
10^3
43
SI Prefix - Deci
10^-1
44
SI Prefix - Centi
10^-2
45
SI Prefix - Milli
10^-3
46
SI Prefix - Micro
10^-6
47
SI Prefix - Nano
10^-9
48
SI Prefix - Pico
10^-12
49
Solids have a ___ shape and are not appreciably ___
definite, compressible
50
Dalton Postulates
1. Each element is composed of extremely small particles called atoms
2. All atoms of a given element are identical to one another in mass and other properties
3. Atoms of an element are not changed into atoms of a different element by chemical reactions; atoms are neither created nor destroyed in chemical reactions
4. Compounds are formed when atoms of more than one element combine; a given compound always has the same relative number and kind of atoms
51
Law of Conservation of Matter: who and what
Lavoisier
The mass of the products is the same as the reactants (matter is neither created nor destroyed but nuclear reactions are different, we don’t look at those)
52
Law of Multiple Proportions: who and what
Dalton
When elements combine, they combine in a ratio of small whole numbers. If two elements can form more than one compound, the ratios of the weight of one element to the weight of the other are small whole numbers
53
Law of Definite Proportions: who and what
Proust
The same compound will always be comprised of its constituent elements in the same proportion by mass.
54
J. J. Thomson's Experiment, what did he suggest
Cathode ray experiment, discovered electrons
55
Robert Millikan's Experiment, what did he suggest
Oil Drop Experiment, calculated the charge of electrons
56
Ernest Rutherford Experiment, what did he suggest?
Gold foil experiment (shot alpha positive particles into gold) , discovered the nucleus AND the nuclear model of the atom
57
Plum Pudding Model, who and what?
Thomson
Positive charge space with electrons (wrong)
58
Nuclear Model
Nucleus with protons and neutrons, electrons were surrounding it (wrong)
59
James Chadwick
Neutron
60
Radioactivity, who?
Becquerel
Spontaneous emission of radiation by an atom
61
Who discovered there were 3 types of radiation, what are they?
Rutherford
Alpha (+)
Beta (-)
Gamma (neutral)
62
Atomic number
Protons
63
Isoelectronic series
Elements with the same number of electrons
64
Isotope
Same element, different amount of neutrons
65
Allotropes
Multiple forms in which an element can exist
ex: carbon is graphite and diamond, only difference is the structure
66
7 diatomic molecules
H2, N2, O2, F2, I2, C2,Br2
HAVE
NO
FEAR
OF
ICE
COLD
BEER
67
Who do we credit for the modern periodic table?
Mendeleev
68
Metals characteristics
-Malleable
-Ductile
-Shiny
-Great conductors
-High melting and boiling points
69
Nonmetal characteristics
Opposite of metals
70
Alkali Metals, group and characteristics
1A; soft, dull metals, REACT VIOLENTLY WITH WATER AND MORE AS U GO DOWN
71
Alkaline Earth Metals, group and characteristics
2A; harder than 1A, react less violently to water
72
Halogen, group and characteristics
7A; naturally occur diatonically and VERY
73
Noble gases, group and characteristics
8A, colorless, monoatomic, inert, unreactive
74
Pair of substances that can be used to illustrate the Law of Multiple Proportions
H2O and CO2
75
What charge does zinc make?
+2
76
What charge does Silver (Ag) make?
+1
77
1 in to cm
2.54
78
Group 6A is known as
Chalcogen
79
Al
Aluminium
80
Ar
Argon
81
Ba
Barium
82
As
Arsenic
83
B
Boron
84
Cd
Cadmium
85
Ca
Calcium
86
C
Carbon
87
Cl
Chlorine
88
Cr
Chromium
89
Co
Cobalt
90
Cu
Copper
91
F
Fluorine
92
Au
Gold
93
H
Hydrogen
93
He
Helium
94
I
Iodine
95
Fe
Iron
96
Kr
Krypton
97
Pb
Lead
98
Li
Lithium
99
Mg
Magnesium
100
Mn
Manganese
101
Hg
Mercury
102
Ne
Neon
103
Ni
Nickel
104
N
Nitrogen
105
O
Oxygen
106
P
Phosphorus
107
K
Potassium
108
Sc
Scandium
109
Se
Selenium
110
Si
Silicon
111
Ag
Silver
112
Na
Sodium
113
Sr
Strontium
114
S
Sulfur
115
Sn
Tin
116
Ti
Titanium
117
V
Vanadium
118
Zn
Zinc
119
Xe
Xenon
120
When naming an ionic compound, monoatomic anions use the ending __
-ide
121
Metal + Nonmetal = ionic and what ending
-ide
122
Metal (with cation charge) + Nonmetal has what ending
-ide
123
Metal (____) + Polyatomic Ion
Cation charge
124
All ionic compounds are crystalline solids with ___ melting points.
High
125
Covalent bonds are formed between 2 ___
Nonmetals
126
Covalent compounds can be ___, ____, or ___ at room temperature
solids, liquids, gases
127
In a binary covalent compound, the ___ electronegative atom is usually listed first.
Less
128
In a covalent compound, the prefix ___ is not used on the first element listed.
Mono-
129
Binary acids consist of __ + nonmetal
Hydrogen
130
In a binary acid, ___ in listed first in the formula
Hydrogen
131
Binary Acid:
Hydrogen + anion+ ___ acid
-ic
132
An oxyacid is a Hydrogen + ____
Polyatomic Anion
133
When naming an oxyacid, hydrogen is listed first in the formula and you can/can't have more than one hydrogen
Can't
134
For oxyacids, -ite is changed to ___ and -ate is changed to __
-ous, -ic
135
What are the 7 strong acids
Hydrochloric Acid - HCl
Hydrobromic Acid - HBr
Hydroiodic Acid - HI
Chloric Acid - HClO4
Perchloric Acid - HClO4
Nitric Acid - HNO3
Sulfuric Acid - H2SO4
136
Acetic Acid formula
CH3COOH
137
Phosphoric Acid formula
H3PO4
138
Chlorous Acid formula
HClO2
139
Hypochlorous Acid formula
ClOH
140
least O - ___
less O - ___
more O - ___
most O - ___
hypo- + -ite
-ite
-ate
per- + -ate
141
Linear alkane means there is only ___ and ___ in the formula
Carbon and hydrogen
142
How to find the number of carbon and hydrogen in a linear alkane?
C(x) H (2x+2)
143
Linear Alkane: prefix - ___
-ane
144
Prefix from 1-10 for Linear Alkanes
1- meth
2- eth
3- prop
4- but
5- pent
6- hex
7- hept
8- oct
9- non
10- dec
145
Functional Groups, what are they?
COOH- ___
NH2- ___
OH- ___
Carboxylic group
Amino group
Hydroxyl group (different than OH-)
146
Molar mass of a compound is the sum of ___
atomic masses of each atom in the compound
147
Mass Percent Formula
[(Mass of part)/ (Mass of whole)] *100
148
Three steps to finding the empirical formula
1. Determine the mass (g) of each element from mass % (assuming you have a 100g sample)
2. Convert the mass of each element to moles and use the atomic mass of each element as the conversion factor
3. Divide all the moles by the smallest number of moles
149
When finding the empirical formula, you can round the number up moles to the nearest whole number when they are within ___ of a whole number.
0.15
150
When a metal and nonmetal react, the __ tends to lose electrons and the ___ tends to gain electrons.
metal, nonmetal
151
Ionic compounds with waters of hydration are named as ___
"ionic compound" prefix-hydrate
