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Freshman > Test 1 Chemistry 116 > Flashcards

Test 1 Chemistry 116 Flashcards

1
Q

Matter

A

A substance that has mass and occupies space

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2
Q

States of Matter

A

Solid, liquid, gas

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3
Q

Mixture (homogenous, heterogeneous)

A

Matter containing more than one type of atom, molecule, etc.

Homogenous: uniform consistency
Heterogenous: non-uniform consistency

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4
Q

Scientific Method

A
  1. Question
  2. Research
  3. Hypothesis
  4. Experiment
  5. Data Analysis
  6. Conclusion
  7. Communication
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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)

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6
Q

Accuracy v.s. Precision

A

Accuracy: how close results how to a known

Precision: how close results are to each other

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7
Q

Sig Fig +/- Rule

A

Answer has the amount of decimal points as the number with the fewest decimal places

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8
Q

Sig Fig x/div Rule

A

Answer has the amount of sig figs as the number with the fewest sig figs

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9
Q

SI Units for mass, length, volume, and temperature

A

kg, m, m^3 (L), kelvin

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10
Q

Fahrenheit Formula

A

F= (9/5 C) +32

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11
Q

Celsius Formula

A

C= (5/9)(F - 32)

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12
Q

Kelvin Formula

A

K= C+273.15

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13
Q

SI Prefix- Mega (M)

A

10^6 from m

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14
Q

SI Prefix- Kilo (k)

A

10^3 from m

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15
Q

SI Prefix- Deci (d)

A

10^-1 from m

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16
Q

SI Prefix- Centi (c)

A

10^-2 from m

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17
Q

SI Prefix- Milli (m)

A

10^-3 from m

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18
Q

SI Prefix- Micro (u)

A

10^-6 from m

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19
Q

SI Prefix- Nano (n)

A

10^-9 from m

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20
Q

SI Prefix- Pico (p)

A

10^-12 from m

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21
Q

Solids have a ___ shape and are not appreciable ___

A

definite, compressible

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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

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23
Q

Initial tentative explanation of an observation

A

Hypothesis

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24
Q

One degree of temperature difference is smallest on the __ scale.

A

Fahrenheit

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25
Q

Freezing point at
C-
F-
K-

A

0, 32, 273.15

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26
Q

Dalton’s Postulates

A
  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
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27
Q

Law of Conservation of Matter

A

The mass of the products= mass of the reactants

Matter is neither created or destroyed (minus nuke reactions)

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28
Q

Law of Multiple Proportions

A

When elements combine, they do so in a ratio of small whole numbers

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29
Q

Who discovered the Law of Multiple Proportions

A

Dalton

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30
Q
A
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31
Q
A
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32
Q

Matter

A

Any substance that has mass and occupies space

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33
Q

Atoms

A

The fundamental building blocks of matter

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34
Q

Types of Mixtures

A

Homogenous: uniform comp. ex: saltwater, sugar water

Heterogenous: non-uniform

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35
Q

Types of Pure Substances

A

Compound: can be chemically decomposed

Element: can’t be chemical decomposed

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36
Q

Initial/tentative explanation of an observation

A

Hypothesis

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37
Q

SI units for mass, length, volume, temperature

A

kg, m, m^3 (L), Kelvin

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38
Q

Celsius Equation

A

C= (5/9)(F-32)

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39
Q

Fahrenheit Equation

A

F= (9/5C)+32

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40
Q

Kelvin Equation

A

K= C+273.15

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41
Q

SI Prefix - Mega

A

10^6

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42
Q

SI Prefix - Kilo

A

10^3

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43
Q

SI Prefix - Deci

A

10^-1

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44
Q

SI Prefix - Centi

A

10^-2

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45
Q

SI Prefix - Milli

A

10^-3

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46
Q

SI Prefix - Micro

A

10^-6

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47
Q

SI Prefix - Nano

A

10^-9

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48
Q

SI Prefix - Pico

A

10^-12

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49
Q

Solids have a ___ shape and are not appreciably ___

A

definite, compressible

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50
Q

Dalton Postulates

A
  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
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51
Q

Law of Conservation of Matter: who and what

A

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)

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52
Q

Law of Multiple Proportions: who and what

A

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

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53
Q

Law of Definite Proportions: who and what

A

Proust

The same compound will always be comprised of its constituent elements in the same proportion by mass.

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54
Q

J. J. Thomson’s Experiment, what did he suggest

A

Cathode ray experiment, discovered electrons

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55
Q

Robert Millikan’s Experiment, what did he suggest

A

Oil Drop Experiment, calculated the charge of electrons

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56
Q

Ernest Rutherford Experiment, what did he suggest?

A

Gold foil experiment (shot alpha positive particles into gold) , discovered the nucleus AND the nuclear model of the atom

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57
Q

Plum Pudding Model, who and what?

A

Thomson

Positive charge space with electrons (wrong)

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58
Q

Nuclear Model

A

Nucleus with protons and neutrons, electrons were surrounding it (wrong)

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59
Q

James Chadwick

A

Neutron

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60
Q

Radioactivity, who?

A

Becquerel

Spontaneous emission of radiation by an atom

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61
Q

Who discovered there were 3 types of radiation, what are they?

A

Rutherford

Alpha (+)
Beta (-)
Gamma (neutral)

62
Q

Atomic number

A

Protons

63
Q

Isoelectronic series

A

Elements with the same number of electrons

64
Q

Isotope

A

Same element, different amount of neutrons

65
Q

Allotropes

A

Multiple forms in which an element can exist

ex: carbon is graphite and diamond, only difference is the structure

66
Q

7 diatomic molecules

A

H2, N2, O2, F2, I2, C2,Br2

HAVE
NO
FEAR
OF
ICE
COLD
BEER

67
Q

Who do we credit for the modern periodic table?

A

Mendeleev

68
Q

Metals characteristics

A

-Malleable
-Ductile
-Shiny
-Great conductors
-High melting and boiling points

69
Q

Nonmetal characteristics

A

Opposite of metals

70
Q

Alkali Metals, group and characteristics

A

1A; soft, dull metals, REACT VIOLENTLY WITH WATER AND MORE AS U GO DOWN

71
Q

Alkaline Earth Metals, group and characteristics

A

2A; harder than 1A, react less violently to water

72
Q

Halogen, group and characteristics

A

7A; naturally occur diatonically and VERY

73
Q

Noble gases, group and characteristics

A

8A, colorless, monoatomic, inert, unreactive

74
Q

Pair of substances that can be used to illustrate the Law of Multiple Proportions

A

H2O and CO2

75
Q

What charge does zinc make?

A

+2

76
Q

What charge does Silver (Ag) make?

A

+1

77
Q

1 in to cm

A

2.54

78
Q

Group 6A is known as

A

Chalcogen

79
Q

Al

A

Aluminium

80
Q

Ar

A

Argon

81
Q

Ba

A

Barium

82
Q

As

A

Arsenic

83
Q

B

A

Boron

84
Q

Cd

A

Cadmium

85
Q

Ca

A

Calcium

86
Q

C

A

Carbon

87
Q

Cl

A

Chlorine

88
Q

Cr

A

Chromium

89
Q

Co

A

Cobalt

90
Q

Cu

A

Copper

91
Q

F

A

Fluorine

92
Q

Au

A

Gold

93
Q

H

A

Hydrogen

93
Q

He

A

Helium

94
Q

I

A

Iodine

95
Q

Fe

A

Iron

96
Q

Kr

A

Krypton

97
Q

Pb

A

Lead

98
Q

Li

A

Lithium

99
Q

Mg

A

Magnesium

100
Q

Mn

A

Manganese

101
Q

Hg

A

Mercury

102
Q

Ne

A

Neon

103
Q

Ni

A

Nickel

104
Q

N

A

Nitrogen

105
Q

O

A

Oxygen

106
Q

P

A

Phosphorus

107
Q

K

A

Potassium

108
Q

Sc

A

Scandium

109
Q

Se

A

Selenium

110
Q

Si

A

Silicon

111
Q

Ag

A

Silver

112
Q

Na

A

Sodium

113
Q

Sr

A

Strontium

114
Q

S

A

Sulfur

115
Q

Sn

A

Tin

116
Q

Ti

A

Titanium

117
Q

V

A

Vanadium

118
Q

Zn

A

Zinc

119
Q

Xe

A

Xenon

120
Q

When naming an ionic compound, monoatomic anions use the ending __

A

-ide

121
Q

Metal + Nonmetal = ionic and what ending

A

-ide

122
Q

Metal (with cation charge) + Nonmetal has what ending

A

-ide

123
Q

Metal (____) + Polyatomic Ion

A

Cation charge

124
Q

All ionic compounds are crystalline solids with ___ melting points.

A

High

125
Q

Covalent bonds are formed between 2 ___

A

Nonmetals

126
Q

Covalent compounds can be ___, ____, or ___ at room temperature

A

solids, liquids, gases

127
Q

In a binary covalent compound, the ___ electronegative atom is usually listed first.

A

Less

128
Q

In a covalent compound, the prefix ___ is not used on the first element listed.

A

Mono-

129
Q

Binary acids consist of __ + nonmetal

A

Hydrogen

130
Q

In a binary acid, ___ in listed first in the formula

A

Hydrogen

131
Q

Binary Acid:
Hydrogen + anion+ ___ acid

A

-ic

132
Q

An oxyacid is a Hydrogen + ____

A

Polyatomic Anion

133
Q

When naming an oxyacid, hydrogen is listed first in the formula and you can/can’t have more than one hydrogen

A

Can’t

134
Q

For oxyacids, -ite is changed to ___ and -ate is changed to __

A

-ous, -ic

135
Q

What are the 7 strong acids

A

Hydrochloric Acid - HCl
Hydrobromic Acid - HBr
Hydroiodic Acid - HI
Chloric Acid - HClO4
Perchloric Acid - HClO4
Nitric Acid - HNO3
Sulfuric Acid - H2SO4

136
Q

Acetic Acid formula

A

CH3COOH

137
Q

Phosphoric Acid formula

A

H3PO4

138
Q

Chlorous Acid formula

A

HClO2

139
Q

Hypochlorous Acid formula

A

ClOH

140
Q

least O - ___
less O - ___
more O - ___
most O - ___

A

hypo- + -ite
-ite
-ate
per- + -ate

141
Q

Linear alkane means there is only ___ and ___ in the formula

A

Carbon and hydrogen

142
Q

How to find the number of carbon and hydrogen in a linear alkane?

A

C(x) H (2x+2)

143
Q

Linear Alkane: prefix - ___

A

-ane

144
Q

Prefix from 1-10 for Linear Alkanes

A

1- meth
2- eth
3- prop
4- but
5- pent
6- hex
7- hept
8- oct
9- non
10- dec

145
Q

Functional Groups, what are they?
COOH- ___
NH2- ___
OH- ___

A

Carboxylic group
Amino group
Hydroxyl group (different than OH-)

146
Q

Molar mass of a compound is the sum of ___

A

atomic masses of each atom in the compound

147
Q

Mass Percent Formula

A

[(Mass of part)/ (Mass of whole)] *100

148
Q

Three steps to finding the empirical formula

A
  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
Q

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.

A

0.15

150
Q

When a metal and nonmetal react, the __ tends to lose electrons and the ___ tends to gain electrons.

A

metal, nonmetal

151
Q

Ionic compounds with waters of hydration are named as ___

A

“ionic compound” prefix-hydrate

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