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CHM 1040 > Exam 1 > Flashcards

Exam 1 Flashcards

1
Q

scientific notation: Measurement

A
  • QUANTITATIVE observation
  • uses numbers and units
  • numbers tells MAGNITUDE
  • unit tells SCALE (unit is slightly more important than #)
  • expresses a # as a product of a # between 1 and 10 and the appropriate power of 10
    ex: 93,000,000 = 9.3 x 10,000,000 = 9.3 x 10^7
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2
Q

10^x

move decimal to the LEFT, exponent is __; move decimal to the RIGHT, exponent is ___

A

positive (+); negative (-)

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3
Q

using scientific notation examples

A 
345 = 3.45 x 10^2
0.0671 = 6.71 x 10^-2
7882 = 7.882 x 10^3
0.0000496 = 4.96 x 10^-5
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4
Q

unit

A

the scale/standard being used to represent the results of a measurement

  • most common systems: English and metric systems
  • internation system (SI)
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5
Q

internation system (SI)

A
  • comprehensive system of units set up by an international agreement
  • units based and derived from metric system
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6
Q

fundamental SI units

A

PHYSICAL QUANTITY UNIT
Mass kg
Length m
Time second
Temp. Kelvin
electric current ampere
amnt. of substance mole

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7
Q

commonly used prefixes in metric system

A

prefix symbol meaning power of 10
mega M 1,000,000 10^6
kilo k 1000 10^3
deci d 0.1 10^-1
centi c 0.01 10^-2
milli m 0.001 10^-3
micro μ 0.000001 10^-6
nano n 0.000000001 10^-9

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8
Q

volume

A
  • measures 3D space by a substance
  • SI unit = m^3
  • commonly measured cm^3
  • 1 mL= 1 cm^3
  • 1 L= 1 dm^3
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9
Q

1 mL= _ cm^3

A

1

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10
Q

1 L= _ dm^3

A

1

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11
Q

length

A 
-fundamental SI unit is meter 
unit         meter equivalent 
km          1000 m or 10^3 m
m            1 m  
dm          0.1 m or 10^-1 m 
cm          0.01 m or 10^-2 m 
mm        0.001 m or 10^-3 m 
μm         0.000001 or 10^-6 m 
nm         0.000000001 or 10^-9
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12
Q

mass

A

-measures matter present in object
-SI unit is kg
1 kg= 2.2046 Ibs
1 Ib= 453.59 g

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13
Q

use __ __ to measure uncertainty

A

sig figs

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14
Q

rules for sig figs

A

1) all nonzero integers ALWAYS count for significance ex: 3456 has 4 sig figs
2) zeros (3 classes of zeros)
a) leading zeros:NEVER count as sig figs
ex: 0.048 has 2 sig figs
b) captive zeros: ALWAYS count as sig figs ex: 16.07 has 4 sig figs
c) trailing zeros: only significant when # HAS A DECIMAL POINT
ex: 9.300 has 4 sig figs; 0.004020 has 4 sig figs; 150 has 2 sig figs

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15
Q

sig figs for x and ÷

A

the # of sig figs for answer is LEAST amount of sig figs u have in the problem

ex: 1.342 x 5.5 = 7.4
* when solving many calculations for 1 problem, don’t convert sig figs until LAST STEP

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16
Q

sig figs for + and -

A

only count decimal places

ex: 23.445 + 7.83 = 31.275 = 31.28
ex: 101 + 1.0 = 102
- always solve from left to right

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17
Q

sig fig question:

4.56 x 7.3679 / 1.006 =

A
  • multiply first, then divide, then find sig figs

answer: 33.4

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18
Q

exponential notation/scientific notation

A

ex: 300 as 3.00 x 10^2 contains 3 sig figs
- advantages
a) # of sig figs can be easily indicated
b) fewer zeros needed to write a very large/very small #

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19
Q

rounding rules

A

when doing many calculations, carry extra digits thru until final result and then round

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20
Q

3 units for measuring temp

A

1) ºF
2) ºC
3) Kelvin (K)

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21
Q

3 major temp scales

A

Farenheit
boiling pt: 212ºF
freezing pt: 32ºF

Celsius
boiling pt: 100ºC
freezing pt: 0ºC

Kelvin
boiling pt: 373 K
freezing pt: 273 K

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22
Q

converting between temp scales

A 
Tk= TºC +273
TºC= Tk-273
TºC= (TºF - 32/1.80)
TºF= 1.80(TºC)+32
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23
Q

K to ºC is

A

-273

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24
Q

density

A

density =mass/volume or D=m/V

  • mass of substance per unit volume of substance
  • common units: g/mL or g/cm^3
  • when mass increases, density increases (directly proportional)
  • when mass is constant and volume decreases, density increases (inversely proportional)
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25
Q

when does ºC = ºF?

A 
x= ºC and ºF
x= 1.80x+32
x-32=1.80x
-32=1.80x-x
-32=x(1.80-1)
x=-32/.80
x=-40
**at -40, ºC=ºF**
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26
Q

matter

A
  • anything occupying space and having mass
  • matter exists in 3 states: s, l, q, and plasma
  • the world is made up of matter and e
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27
Q

solid

A
  • rigid
  • doesn’t change shape
  • has a fixed volume and shape
  • ex: ice cube, rock, diamond, phones, chair
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28
Q

liquid

A
  • has a definite volume
  • will take shape of container
  • ex: car gas, water, alcohol, blood, ocean
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29
Q

gas

A
  • no fixed volume or shape
  • takes shape and volume of a container
  • ex: air, helium, O2, atmosphere
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30
Q

plasma

A

gas so supercharged that it has liquid

ex: lightning, comets, neon signs

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31
Q

physical properties

A
  • characteristic that are directly observable and unique to a substance
  • ex: odor, volume, color, state (s,l,g,p), density, boiling pt, melting pt
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32
Q

chemical properties

A
  • a substance’s ability to make new substances
  • characteristics that determine how the composition of matter changes as a result of contact w/ other matter/influence of e
  • characteristics that describe behavior of matter
  • ex: flammability, rusting of steel, toxicity, enthalpy, chemical stability, reactivity, digestion of food
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33
Q

ethyl alcohol at 78ºC boiling point is a __ property

A

physical

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34
Q

hardness of a rock is a __ property

A

physical

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35
Q

sugar fermenting to form ethyl alcohol is a __ property

A

chemical

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36
Q

physical change

A
  • change in 1 or more properties of a substance and not in its chemical composition
  • ex: boiling pt or freezing water
  • 3 states of water: in all phases, water mols are still intact; motion of mols and distance between them change
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37
Q

chemical change

A
  • given substance becomes a new substance w/ diff properties and diff composition
  • ex: Bunsen burner, methane reacts w/O2 to make CO2 and H2O, baking a cake, bleaching teeth (rxn happening), digesting food
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38
Q

crushing salt is a __ change

A

physical

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39
Q

burning wood is a __ change

A

chemical

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40
Q

dissolving sugar in water is a __ change

A

physical

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41
Q

melting a popsicle is a __ change

A

physical

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42
Q

element

A

a substance that CANNOT be broken down into other substances by chemical methods

  • ex: Fe, Al, O2, H2
  • all matter in world around us has elements
  • almost 99% of mass of human body is made up of 6 elements (highest to lowest O2, C, H2, N, Ca, P)
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43
Q

compound

A

substance made of a given combination of elements that CAN be broken down into those elements by chemical methods

  • ex: water, CO2, table sugar (C6H22O11)
  • ALWAYS contains atoms of diff elements
  • ALWAYS has the same composition/same combination of atoms
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44
Q

H2O, N2O4, NaOH, MnO2, and HF are ALL ___

A

compounds

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45
Q

pure substances

A
  • always have same composition
  • either elements or compounds
  • ex: pure water (H2O), CO2, H2, gold (Au)
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46
Q

mixtures

A
  • 2 or more pure substances
  • have variable composition
  • ex: wood, wine, coffee
  • can be separated into pure substances that are elements and/or compounds
  • 2 types: homogenous and heterogeneous
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47
Q

homogeneous mixture

A
  • substance that is same throughout
  • consists of visibly INDISTINGUISHABLE parts
  • aka a SOLUTION
  • doesn’t vary in comp. from 1 region to another
  • ex: air around us, brass, mashed potatoes, chocolate milk, table salt in water
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48
Q

heterogeneous mixtures

A
  • consists of visibly DISTINGUISHABLE parts
  • contains regions that have diff properties from other regions
  • ex: oil and vinegar dressing, salad, sand in water, soup, chocolate chip cookies
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49
Q

organization of matter

A

MATTER
homogeneous mixtures heterogeneous mixtures
pure substances
elements

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50
Q

the elements

A
  • 118 known
    a) 88 occur naturally
    b) rest have been made in labs
  • vary in abundance
    a) only 9 elements account for most of the compounds found in Earth’s crust
    b) these 9 elements account for over 98% of the total mass of the Earth’s crust, oceans, and atmosphere
  • list of elements found in living matter is very diff from those found in the Earth’s crust
    a) O2, N, and C forms the basis for all biologically important molecules
    b) trace elements present in the body are very crucial
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51
Q

compound

A

district substance composed of atoms of 2 or more elements

-always contains exactly the sam relative masses of those elements

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52
Q

chemical formulas

A

express types of atoms and # of each type in each unit, or molecule, of a given compound

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53
Q

rules for writing formulas

A
  • each atom present is represented by its element symbol
  • # of each type of atom is indicated by a subscript written to the right of the element symbol
  • when only 1 atom of a given type is present, the subscript “1” is not written
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54
Q

what are atoms made up of?

A

e-, protons, and neutrons

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55
Q

electrons

A

e-; (-) charged; found outside nucleus

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56
Q

protons

A

(+) charged; found inside nucleus; has equal magnitude to e-

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57
Q

neutrons

A

no charge; found in nucleus; virtually same mass as proton

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58
Q

protons and neutrons have the same __

A

mass

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59
Q

mass charge of the e-, proton, and neutron

A

particle relative mass relative charge
e- 1 1-
proton 1836 1+
neutron 1839 none

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60
Q

why do diff atoms have diff chemical properties?

A
  • the chemistry of an atom arises from its e-
  • e- are part of atoms that intermingle when atoms combine to make molecules
  • it’s the # of e- that really determines chemical behavior
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61
Q

the chemistry of an atom arises from its __

A

electrons

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62
Q

isotopes

A

diff # of neutrons

  • atoms w/ the same # of protons but diff # of neutrons
  • show almost identical chem. properties
  • chemistry of an atom is due to its e-
  • in nature, elements are usually found as a mixture of isotopes
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63
Q

elements on periodic table are the most ABUNDANT __

A

isotopes

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64
Q

isotope symbol

A 
A
   X
Z
X= the chemical symbol of element 
A= mass # (# of protons + # of neutrons)
Z= atomic # (# of protons)
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65
Q

the periodic table

A

shows all of the known elements in the order of increasing atomic #

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66
Q

groups/families

A

elements in same VERTICAL columns and have similar chemical properties

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67
Q

periods

A

HORIZONTAL rows of elements

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68
Q

metals

A

LEFT of staircase

-most elements are these

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69
Q

non-metals

A

RIGHT of staircase

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70
Q

metalloids

A

ON the staircase

-have some metallic and some non-metallic properties

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71
Q

what are the metalloids?

A 
Boring Silly Germs Are Ants Telling Politics
Boron (B)
Silicon (Si)
Germanium (Ge)
Arsenic (As)
Antimony (Sb)
Tellurium (Te)
Polonium (Po)
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72
Q

** what are the four physical properties of metals? **

A

1) efficient conduction of heat and electricity
2) malleability (aluminum foil)
- they can be hammered into thin sheets
3) ductility
- they can be pulled into wires
- can be molded
4) lustrous appearance (shiny)

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73
Q

physical properties of non-metals

A
  • lack properties of metals
  • exhibit more variation in properties
  • can be g, l, s @ room temp
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74
Q

physical properties of metalloids

A

exhibit a mixture of metallic and non-metallic properties

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75
Q

natural states of the elements

A

-most are reactive
-not generally found in pure form
-exceptions: noble metals ( gold, platinum, silver)
noble gasses: group 8

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76
Q

diatomic molecules

A
  • so reactive they bind to themselves
  • 7 diatomic molecules
  • Nitrogen gas contains N2 molecules
  • Oxygen gas contains O2 molecules
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77
Q

7 diatomic molecules

A

I Bring Clay For Our New Home

  • Iodine (I2): lustrous, dark purple solid
  • Bromine (Br2): reddish-brown liquid
  • Chlorine (Cl2): pale green gas
  • Fluorine (F2): pale yellow gas
  • Oxygen (O2): pale blue gas
  • Nitrogen (N2): colorless gas
  • Hydrogen (H2): colorless gas
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78
Q

ions

A
  • atom’s not neutral
  • atom w a charge
  • elements become ions
  • imbalance of e-
  • atoms can form ions by gaining/losing e-
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79
Q

cations

A

metals tend to lose 1 or more e- to form (+) ions

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80
Q

anions

A

nonmetals tend to gain 1 or more e- to form (-) ions

-name changes to end in -ide

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81
Q

ion charges & the periodic table

A

the ion that a particular atom will form can be predicted from the atom’s position on the periodic table

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82
Q

ion charges and the periodic table chart

A

Group or Family Charge
Alkali Metals (1A) 1+
Alkaline Earth Metals (2A) 2+
Halogens (7A) 1-
Noble Gasses (8A) 0

*group 1: +1
 group 2: +2
 group 3: +3
 group 6: -2
 group 7: -1
 group 8: 0
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83
Q

an ion with a 3+ charge w/ 24 e- is

84
Q

ion X+ has 54 e- and 78 neutrons. What is the mass number?

85
Q

periodic table: Hydrogen

A

H
alkali metals
group 1
*diatomic

86
Q

periodic table: Lithium

A

Li
alkali metals
+1

87
Q

periodic table: Sodium

A

Na
alkali metals
+1

88
Q

periodic table: Potassium

A

K
alkali metals
+1

89
Q

periodic table: Rubidium

A

Rb
alkali metals
+1

90
Q

periodic table: Cesium

A

Cs
alkali metals
+1

91
Q

periodic table: Francium

A

Fr
alkali metals
+1

92
Q

periodic table: Beryllium

A

Be
alkaline earth metals
+2

93
Q

periodic table: Magnesium

A

Mg
alkaline earth metals
+2

94
Q

periodic table: Calcium

A

Ca
alkaline earth metals
+2

95
Q

periodic table: Strontium

A

Sr
alkaline earth metals
+2

96
Q

periodic table: Barium

A

Ba
alkaline earth metals
+2

97
Q

periodic table: Radium

A

Ra
alkaline earth metals
+2

98
Q

periodic table: Scandium

A

Sc

transition metal

99
Q

periodic table: Yttrium

A

Y

transitional metal

100
Q

periodic table: Titanium

A

Ti

transitional metal

101
Q

periodic table: Zirconium

A

Zr

transitional metal

102
Q

periodic table: Hafnium

A

Hf

transitional metal

103
Q

periodic table: Rutherfordium

A

Rf

transitional metal

104
Q

periodic table: Vanadium

A

V

transitional metal

105
Q

periodic table: Niobium

A

Nb

transitional metal

106
Q

periodic table: Tantalum

A

Ta

transitional metal

107
Q

periodic table: Dubnium

A

Db

transitional metal

108
Q

periodic table: Chromium

A

Cr

transitional metal

109
Q

periodic table: Molybdenum

A

Mo

transitional metal

110
Q

periodic table: Tungsten

A

W

transitional metal

111
Q

periodic table: Seaborgium

A

Sg

transitional metal

112
Q

periodic table: Manganese

A

Mn

transitional metal

113
Q

periodic table: Technetium

A

Tc

transitional metal

114
Q

periodic table: Rhenium

A

Re

transitional metal

115
Q

periodic table: Bohrium

A

Bh

transitional metal

116
Q

periodic table: Iron

A

Fe

transitional metal

117
Q

periodic table: Ruthenium

A

Ru

transitional metal

118
Q

periodic table: Osmium

A

Os

transitional metal

119
Q

periodic table: Hassium

A

Hs

transitional metal

120
Q

periodic table: Cobalt

A

Co

transitional metal

121
Q

periodic table: Rhodium

A

Rh

transitional metal

122
Q

periodic table: Iridium

A

Ir

transitional metal

123
Q

periodic table: Meitnerium

A

Mt

transitional metal

124
Q

periodic table: Nickel

A

Ni

transitional metal

125
Q

periodic table: Palladium

A

Pd

transitional metal

126
Q

periodic table: Platinum

A

Pt

transitional metal

127
Q

periodic table: Copper

A

Cu

transitional metal

128
Q

periodic table: Silver

A

Ag

transitional metal

129
Q

periodic table: Gold

A

Au

transitional metal

130
Q

periodic table: Zinc

A

Zn

transitional metal

131
Q

periodic table: Cadmium

A

Cd

transitional metal

132
Q

periodic table: Mercury

A

Hg

transitional metal

133
Q

periodic table: Boron

A

B
+3
metalloid

134
Q

periodic table: Aluminum

A

Al
+3
metal

135
Q

periodic table: Gallium

136
Q

periodic table: Indium

137
Q

periodic table: Thallium

138
Q

periodic table: Carbon

A

C

nonmetal

139
Q

periodic table: Silicon

A

Si

metalloid

140
Q

periodic table: Germanium

141
Q

periodic table: Tin (stannum)

142
Q

periodic table: Lead (Plumbum)

143
Q

periodic table: Nitrogen

A

N
-3
non-metal
*diatomic

144
Q

periodic table: Phosphorus

A

P
-3
nonmetal

145
Q

periodic table: Arsenic

A

As
-3
metalloid

146
Q

periodic table: Antimony

A

Sb
-3
metalloid

147
Q

periodic table: Bismuth

148
Q

periodic table: Oxygen

A

O
-2
nonmetal
*diatomic

149
Q

periodic table: Sulfur

A

S
-2
nonmetal

150
Q

periodic table: Selenium

A

Se
-2
nonmetal

151
Q

periodic table: Tellurium

A

Te
-2
metalloid

152
Q

periodic table: Polonium

A

Po
-2
metalloid

153
Q

periodic table: Fluorine

A

F
-1
halogens
*diatomic

154
Q

periodic table: Chlorine

A

Cl
-1
halogens
*diatomic

155
Q

periodic table: Bromine

A

Br
-1
halogens
*diatomic

156
Q

periodic table: Iodine

A 
I
group 7
-1
halogens
*diatomic
157
Q

periodic table: Astatine

A

At
-1
halogens

158
Q

periodic table: Helium

A

He
0
noble gases

159
Q

periodic table: Neon

A

Ne
0
noble gases

160
Q

periodic table: Argon

A

Ar
0
noble gases

161
Q

periodic table: Krypton

A

Kr
0
noble gases

162
Q

periodic table: Xenon

A

Xe
0
noble gases

163
Q

periodic table: Radon

A

Rn
0
noble gases

164
Q

Which of the steps in the scientific method is missing from the following situation?
“Your instructor is holding a balloon and quickly inhales some of the gas inside the balloon. He then speaks and his voice changes to a high-pitched sound (and sounds quite funny!). He then asks you to determine what gas was inside the balloon that he inhaled. Based on your observations, you conclude that the gas must be helium.”

A

perform experiments

165
Q

what is chemistry?

A

The science that deals with the materials of the universe and the changes that these materials undergo.

  • The central science
    • Understanding most other fields of science requires an understanding of chemistry.
166
Q

solving problems w/ a scientific approach

A

1.Recognize the problem and state it clearly.
a)Making an observation.
2.Propose possible solutions to the problem or possible explanations for the observation.
a)Formulating a hypothesis.
3.Decide which of the solutions is the best or decide whether the explanation proposed is reasonable
.a)Performing an experiment.

167
Q

science

A

a framework for gaining and organizing knowledge.
•a plan of action —a procedure for processing and understanding certain types of information.
•Scientists are always challenging our current beliefs about science, asking questions, and experimenting to gain new knowledge.
-Scientific method is needed.

168
Q

Which of the following correctly expresses 7,882 in scientific notation?

A

7.882 × 10^3

169
Q

Which of the following correctly expresses 0.0000496 in scientific notation?

A

4.96 × 10^–5

170
Q

Choose the statement(s) that contain improper use(s) of commonly used units

A

A basketball is 7 m tall

A nickel is 6.5 cm thick

171
Q

What data would you need to estimate the money you would spend on gasoline to drive your car from New York to Los Angeles? Provide estimates of values and a sample calculation.

A

Distance between New York and Los Angeles is 2500 miles
– Average gas mileage is 25 miles per gallon
– Average cost of gasoline is $3.25 per gallon
2500 mi x 1 gal/25 mi x $3.25/1 gal = $325

172
Q

The normal body temperature for a dog is approximately 102°F. What is this equivalent to on the Kelvin temperature scale?

173
Q

A certain mineral has a mass of 17.8 g and a volume of 2.35 cm^3. What is the density of this mineral?

A

7.57 g/cm^3

174
Q

What is the mass of a 49.6 mL-sample of a liquid, which has a density of 0.85 g/mL?

175
Q

If an object has a mass of 243.8 g and occupies a volume of 0.125 L, what will be the density of this object in g/cm^3?

A

1.95 g/cm^3

176
Q

Copper has a density of 8.96 g/cm^3. 75.0 g of copper is added to 50.0 mL of water in a graduated cylinder. Determine the volume reading to which the water level in the cylinder will rise.

177
Q

Which of the following are examples of a chemical change?

A

Burning of wood

178
Q

Which of the following is a homogeneous mixture?

179
Q

A certain isotope X contains 23 protons and 28 neutrons
•What is the mass number of this isotope?
•Identify the element

A

Mass Number = 51

Vanadium

180
Q

compounds that contain ions: ionic compounds

A
  • ions combine to form ionic compounds
  • properties of ionic compounds:
    1. high melting pts
    2. conduct e-
    • if melted
    • if dissolved in water
  • transfer e-
  • strongest bonds
  • bond between a metal and a nonmetal
  • electrically neutral
  • charges on anions and cations in compound must = 0
181
Q

compounds that contain ions: formulas for ionic compounds

A
  • write cation element symbol followed by anion element symbol
  • # of cations and anions must be correct for their charges to = 0
  • if they don’t = 0, u must balance them
    ex: MgCl2 = Mg (2+) and 2( Cl(-1) ) -> Cl (-2) = compound net charge of 0 for MgCl2
182
Q

name the ionic compound NaBr

A

sodium bromide

183
Q

name the ionic compound calcium fluoride

184
Q

name the ionic compound KCl

A

potassium chloride

185
Q

name the ionic compound lithium iodide

186
Q

name the ionic compound MgO2

A

magnesium oxide

187
Q

e- give __; protons and neutrons give __

A

size; weight

188
Q

out of all 3, which is the smallest subatomic particle?

189
Q

what are the 3 steps of the scientific method?

A

1) make an observation
2) form a hypothesis
3) perform experiment
-leads u to
theory: answers “why?”, leads to more questions
the law: “this is what happened”, doesn’t lead to more questions

190
Q

sig fig question: 1.5 +3.000 - 4

A

4.5- 4 = 0.5 = 5 x 10^-1

191
Q

1 kg = __ g

192
Q

1000 mL= ___ L

193
Q

100 cm= __ m

194
Q

1000 mg= __ g

195
Q

1 mL= __ cm^3

196
Q

100 mm= __ m

197
Q

1 lb= __ g

198
Q

1 kg= _ Ibs

199
Q

1 in = __ cm

200
Q

periodic table: darmstadtium

A

Ds

transition metal

201
Q

periodic table: roentgenium

A

Rg

transition metal

202
Q

group 1

+1

A 
alkali metals
Highly Nasty Kids Rub Cats 
Li (lithium)
Na (sodium)
K (potassium)
Rb (rubidium)
Cs (cesium)
203
Q

group 2

+2

A 
alkaline earth metals
Beer Mugs Can Serve Bar Rats
beryllium (Be)
magnesium (Mg)
calcium (Ca)
strontium (Sr)
barium (Ba)
radium (Ra)
204
Q

group 3

+3

A 
Bears Always Give In
boron (B)
aluminum (Al)
gallium (Ga)
indium (In)
205
Q

group 6

-2

A 
Old Soldiers Seem Tense
oxygen (O)
sulfur (S)
seaborgium (Se)
tellurium (Te)
206
Q

group 7

-1

A 
halogens 
“Floor Cleaner Broken?” I Asked
fluorine (F)
chlorine (Cl)
bromine (Br)
iodine (I)

CHM 1040 (6 decks)

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