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CHEM 110 - MIDTERM #1 Flashcards

1
Q

What kind of science is Chemistry?

A

Central Science - it joins together all the sciences (physics & biology)

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2
Q

What is the scientific method?

A

Systematic approach to research (observation -> representation -> interpretation)

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3
Q

What is the difference between law and theory?

A

Law: concise statement of a relationship between phenomena that is always the same under the same conditions (F = ma)
Theory: unifying principle that explains a body of facts and/or those laws based on them (atomic theory)

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4
Q

Chemistry is the study of ______.

A

Matter

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5
Q

What is a substance?

A

Form of matter that has a definite composition and distinct properties (Ex: H2O)

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6
Q

What is a mixture?

A

Combination of 2 or more substances in which the substances retain their distinct identities

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7
Q

Difference between homogenous mixture & heterogenous mixture?

A

Homogenous mixture: mixture composition is the same throughout
Hetereogenous mixture: composition is not uniform throughout

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8
Q

What is are some examples of a homogenous mixture?

A

Air, Sea Water, Wine

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9
Q

What are some examples of heterogenous mixtures?

A

Chicken noodle soup, sand, oil & water

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10
Q

What is the physical means of separating a mixture?

A

Does not change the chemical composition of a substance (ie. distillation, ice melting, magnet)

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11
Q

What is the chemical means of separating a mixture?

A

Changing the chemical composition or identity of the substance(s) involved

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12
Q

An element cannot be separated into simpler substances by _______ means.

A

chemical

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13
Q

What is a compound?

A

A substance composed of atoms of two or more elements chemically united in fixed proportions

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14
Q

A compound can be separated into their pure elements by _____ means.

A

Chemical

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15
Q

What’s the difference between a mixture and a substance?

A

Mixture: combination of substances that can be separated by physical methods to form substances
Substances: form of matter with distinct properties composted of compounds and elements

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16
Q

Compounds can be separated via chemical methods to form ____.

A

Elements

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17
Q

3 States of Matter

A

Solid: dense shape
Liquid: more degrees of freedom
Gas: no shape, but occupy space all throughout

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18
Q

What is an example of chemical change?

A

Hydrogen burning in air to form water

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19
Q

What’s the difference between extensive and intensive properties?

A

Extensive: dependent on amount of matter
Intensive: does NOT dependent on matter

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20
Q

What are examples of extensive properties?

A

Mass, volume, length

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21
Q

What are examples of intensive properties?

A

Density, Color, Temperature

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22
Q

What is matter?

A

Anything that occupies space and has mass

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23
Q

What is weight?

A

Force that gravity exerts on an object

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24
Q

What SI unit measures the amount of substance?

A

Mole (mol)

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25
Kilo-
1000 (10^3)
26
Milli-
1/1000 (10^-3)
27
Micro-
1/(10^6)
28
deci-
1/10 (10^-1)
29
centi-
1/100 (10^-2)
30
nano-
10^-9
31
mega-
10^6
32
pico-
10^-12
33
What is volume?
SI derived unit for volume is cubic meter (m^3) where 1 mL = 1 cm^3
34
What is density?
SI derived unit for density is kg/m^3 D = mass/volume
35
What are the units for density?
g/mL or g/cm^3
36
How do we find Kelvin (K) from using Celsius?
K = C + 273.15
37
What is 0 Celsius in Kelvin?
273.15
38
How do we find the degrees in Fahrenheit?
F = 9/5 x C + 32
39
What is scientific notation?
A convenient way of showing the # of significant figures in a value
40
When you multiply you ___ exponents.
add
41
When you divide exponents, you ___ exponents.
subtract
42
What are significant figures?
Any digit that is not zero ~ provides uncertainty and accuracy of a measurement
43
What is the rule for addition/subtraction with # of sig figs?
The answer cannot have more digits to the right of the decimal point than any of the original numbers (83.3333 + 1.1 = 90.4)
44
What is the rule for multiplication/division of sig figs?
The # of sig figs must be set by the original number that has the smallest number of sig figs (4.51 + 8.7777777 = 16.6)
45
What is the difference between accuracy and precision?
Accuracy: how close a measurement is to the true value Precision: how close a set of measurements are to each other
46
Give an example of a compound
Sugar, water
47
Water boiling is an example of ___ change
physical
48
fertilizers help to increase agricultural production is an example of ____ change
chemical
49
the flashlight beam slowly gets dimmer and finally goes out is an example of ___ change
chemical
50
What is Dalton's Atomic Theory?
1) Elements are composed of atoms 2) All atoms of an element are identical, have same size, mass and chemical properties 3) Compounds are composed of atoms of more than one element 4)A chemical reaction is the rearrangement of atoms (not creation or destruction - law of conservation of mass)
51
What is the law of conservation of mass?
Mass is not created or destroyed
52
What is Dalton's Law of Multiple Proportions?
If 2 elements form more than one compound - the ratio of the masses of the 2nd element can be reduced to whole numbers
53
What was the finding of Rutherford's Experiment (1908)?
1) Atoms positive charge is concentrated in the nucleus 2) Protons have an opposite charge (+) of an electron (-) 3) Mass of a proton = 1840 x mass of e- (1.67 x 10^-24 g) = protons are bigger than electrons
54
What is the atomic number (Z)?
number of protons in a nucleus and determines the identity of an element
55
What is the mass number (A)?
number of protons + neutrons
56
What are isotopes?
Atoms of the element with different numbers of neutrons in their nuclei
57
What is the first group and respective charge in the period table?
Alkali Metals (+1)
58
What is the second group of the periodic table with their respective charge?
Alkaline Earth Metals (+2)
59
What is the name of the 3rd-12th group in the periodic table?
Transition metals (varying charges)
60
What is the name of the 7th group of the periodic table and their respective charges?
Halogens (-1)
61
What is the name of the last group of the periodic table?
Noble gases
62
What is the difference between a period and a group?
period = row in the periodic table group = column in the periodic table
63
What is a molecule?
Aggregate of 2 or more atoms held by chemical forces
64
What is an example of a diatomic molecule?
N2, H2, CO, HCl (2 atoms)
65
What is an example of a polyatomic molecule?
O3, CH4 (more than 2 atoms)
66
What is an ion?
Atom(s) with a net positive or negative charge
67
What are the two types of ions?
Anion and cation
68
What is the difference between cation and anions?
Cation: net positive charge (lose an electron) Anion: net negative charge (gain an electron)
69
What is an example of a monatomic ion?
Na+, Cl-
70
What are the two types of formulas and what are their differences?
Molecular (exact number of atoms of each element in the smallest unit of a substance) & empirical (simplest whole number ratio of atoms in a substance)
71
An example of molecular and empirical formula
C6H12O6 (molecular) CH2O (empirical)
72
What are ionic compounds held together by?
Electrostatic forces (+) and (-) charges
73
Ionic compounds are generally formed with a ____ and ____
metal, nonmetal
74
What is an example of an ionic compound?
Na+Cl-
75
What is the chemical nomenclature of ionic compounds?
The anion (nonmetal), add "'-ide" to element name
76
What is the chemical name for K2O?
Potassium oxide
77
How do we name transition metal ionic compounds?
Indicate the charge on metal with roman numerals
78
How do we name FeCl2?
Iron (II) chloride
79
Name Monatomic Atom for S?
Sulfide
80
Name Monatomic Atom for N?
Nitride
81
Name Monatomic Atom for P?
Phosphide
82
What is an inorganic cation?
NH4 (ammonium)
83
Cu(NO3)2 name?
Copper (II) nitrate
84
KH2PO4 name?
Potassium dihydrogen phosphate
85
Calcium phosphate formula?
Ca3(PO4)2
86
What do molecular compounds consist of?
Nonmetals/nonmetals + metalloids (they are held together by covalent bonds and made up of discrete, individual molecules)
87
Common molecular compound?
H2O, CH4, NH3
88
____ compounds use Greek prefixes & the last element ends in ___ for chemical nomenclature
Molecular, -ide
89
1
Mono-
90
2
Di-
91
3
Tri-
92
4
Tetra-
93
5
Penta-
94
6
Hexa-
95
7
Hepta
96
9
Nona-
97
Deca-
10
98
NF3 name?
Nitrogen trifluoride
99
N2O name?
dinitrogen monoxide
100
SiCl4 name?
Silicon tetrachloride
101
P4O10 name?
Tetraphosphorus Decoxide
102
What is an acid?
Substance that yields H+ ions when dissolved in water
103
HF name?
hydrofluoric acid
104
HCl name?
Hydrochloric acid
105
HBr name?
Hydrobromic acid
106
HI name?
hydroiodic acid
107
HCN name?
hydrocyanic acid
108
H2S name?
Hydrosulfuric acid
109
What is an oxoacid?
An acid that contains hydrogen, oxygen, and another element
110
Examples of oxoacids?
Nitric acid (HNO3), Carbonic Acid (H2CO3), Phosphoric acid (H3PO4)
111
H2SO4 name?
Sulfuric acid (Oxoacid)
112
HClO3- name?
Chloric Acid (Oxoacid)
113
Naming Oxoanions?
1) Anion ends in "-ate" when the H ions are removed from the "ic" acid 2) Anion ends in "ite" when the H ions are removed from the "-ous" acid 3) Number of H atoms present are indicated with anion names (dihydrogen phosphate H2PO4)
114
HClO4 name?
Perchloric acid
115
HClO3 name?
Chloric acid
116
HClO2 name?
Chlorous acid
117
HClO name?
Hypochlorous acid
118
Why does the nomenclature vary with perchloric acid, chloric acid, chlorous acid and hypochlorous acid?
# of oxygens vary, corresponding anion vary
119
H3PO3 name?
Phosphorous acid
120
HIO4 name?
Periodate
121
What is a base?
A substance that yields hydroxide ions (-OH) when dissolved in water
122
NaOH name and ID?
Sodium hydroxide, base
123
What is a hydrate?
A compound that has a specific number of water molecules attached to them
124
LiCl x H2O name and ID?
Lithium chloride monohydrate
125
BaCl2 x 2H2O name and ID?
Barium chloride dihydrate
126
H2O name?
dihydrogen monoxide
127
CaO name?
Calcium oxide
128
Simplest type of organic compound?
Hydrocarbon
129
Protons and neutrons are ____ than electrons
larger in mass (same with each other)
130
Mg(HCO3)2 name?
Magnesium bicarbonate
131
HBrO4 name?
Perbromic acid
132
HrBrO3 name?
Bromic acid
133
HBrO2 name?
Bromous acid
134
HBrO name?
Hypobromous acid
135
HIO4 name
Periodic acid
136
HIO3 name
Iodic acid
137
HIO2 name
Iodous acid
138
HIO name
Hypoiodous acid
139
H2SO3 name
Sulfurous acid
140
HNO3 name
Nitric acid
141
HNO2 name
Nitrous acid
142
H3PO4 name
Phosphoric acid
143
H3PO3
phosphorous acid
144
What is atomic mass?
The mass of an atom in atomic mass units (1 atom C = 12 amu)
145
What is average atomic mass?
Weighted average of all naturally occurring isotopes of the element (based on relative abundance) To solve: 1) Convert percentage given of isotope into a decimal (60.0% -> 0.600) 2) Multiply decimal by amount of grams given of isotope 3) Add the atomic masses (products) together to find the average within the element
146
What is a mole?
A unit to count number of particles - contains as many elementary entities as there are atoms in exactly 12 grams of 12C
147
Avogadro's number is used to find the number of ____ of a compound/element
atoms/particles
148
What is molar mass?
Mass of 1 mole of anything in grams
149
How do we convert from mass to atoms of an element?
Mass (g) --> Molar mass --> Moles --> Avogadro's number--> Atoms
150
What is the molecular mass (molecular weight)?
Sum of the atomic masses (in amu) in a molecule
151
What is the formula mass?
Sum of atomic masses (in amu) in a formula unit of an ionic compound
152
What is the percent composition and how do we calculate it?
The amount of an element in a compound; calculated by: 1) Find the atomic mass of the element with respect to its coefficient in the equation 2) Divide atomic mass by the molar mass of the compound 3) Multiply the product by 100 to find the percentage
153
How would we find the empirical formula given the percent composition?
1) Convert the percent given into grams of an element (40.0% -> 40.0 grams of C) 2) Use the grams to find number of moles (by dividing by molar mass of compound) 3) Identify the smallest amount of moles and divide the other products by the smallest number to find a smallest compound ratio 4) If needed to achieve a whole number, multiply all the products by a common integer to achieve a whole number 5) Write out empirical formula with the subscripts :)
154
We cannot use the ____ to read a chemical reaction. Only moles and molecules
Mass (g)
155
Stoichiometric coefficients are consist with ____, not ____.
moles, grams
156
What is the limiting reagent?
The reactant used up first in the reaction

CHEM 110 (4 decks)

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