Chapter 1 Flashcards
Essential Ideas
1
Q
accuracy
A
how closely a measurement aligns with a correct value
2
Q
atom
A
smallest particle of an element that can enter into a chemical combination
3
Q
Celsius (°C)
A
unit of temperature; water freezes at 0 °C and boils at 100 °C on this scale
4
Q
chemical change
A
change producing a different kind of matter from the original kind of matter
5
Q
chemical property
A
behavior that is related to the change of one kind of matter into another kind of matter
6
Q
chemistry
A
study of the composition, properties, and interactions of matter
7
Q
compound
A
pure substance that can be
decomposed into two or more elements
8
Q
cubic centimeter (cm3 or cc)
A
volume of a cube with an edge length of exactly 1 cm
9
Q
cubic meter (m3)
A
SI unit of volume
10
Q
density
A
ratio of mass to volume for a substance or object
11
Q
dimensional analysis
A
(also, factor-label method) versatile mathematical approach that can be applied to computations ranging from simple unit conversions to more complex, multi-step calculations involving several different quantities
12
Q
element
A
substance that is composed of a single
type of atom; a substance that cannot be decomposed by a chemical change
13
Q
exact number
A
number derived by counting or by definition
14
Q
extensive property
A
property of a substance that depends on the amount of the substance
Mass
Length
Volume
15
Q
Fahrenheit
A
unit of temperature; water freezes at 32 °F and boils at 212 °F on this scale
16
Q
gas
A
state in which matter has neither definite volume nor shape
17
Q
heterogeneous mixture
A
combination of substances with a composition that varies from point to point
18
Q
homogeneous mixture
A
(also, solution) combination of substances with a composition that is uniform throughout
19
Q
hypothesis
A
tentative explanation of observations that acts as a guide for gathering and checking information
20
Q
intensive property
A
property of a substance that is independent of the amount of the substance
Density
Temperature
Color
21
Q
kelvin (K)
A
SI unit of temperature;
273.15 K = 0 ºC
22
Q
kilogram (kg)
A
standard SI unit of mass;
1 kg = approximately 2.2 pounds
23
Q
law
A
statement that summarizes a vast number of experimental observations, and describes or predicts some aspect of the natural world
24
Q
law of conservation of matter
A
when matter converts from one type to another or changes form, there is no detectable change in the total amount of matter present
25
length
measure of one dimension of an object
26
liquid
state of matter that has a definite volume but
indefinite shape
27
liter (L)
(also cubic decimeter) unit of volume;
1 L = 1,000 cm3
28
macroscopic domain
realm of everyday things that are large enough to sense directly by human sight and touch
29
mass
fundamental property indicating amount of
matter
30
matter
anything that occupies space and has mass
31
meter (m)
standard metric and SI unit of length;
1 m = approximately 1.094 yards
32
microscopic domain
realm of things that are
much too small to be sensed directly
33
milliliter (mL)
1/1,000 of a liter = 1 cm3
34
mixture
matter that can be separated into its components by physical means
35
molecule
bonded collection of two or more atoms of the same or different elements
36
physical change
change in the state or properties of matter that does not involve a change in its chemical composition ie **condensation**
37
physical property
characteristic of matter that is not associated with any change in its chemical composition
38
plasma
gaseous state of matter containing a large
number of electrically charged atoms and/or molecules
39
precision
how closely a measurement matches the same measurement when repeated
40
pure substance
homogeneous substance that has a constant composition
41
rounding
procedure used to ensure that calculated
results properly reflect the uncertainty in the
measurements used in the calculation
42
scientific method
path of discovery that leads from question and observation to law or hypothesis to theory, combined with experimental verification of the hypothesis and any necessary modification of the theory
43
second (s)
SI unit of time
44
SI units (International System of Units)
standards fixed by international agreement in the International System of Units (Le Système International d’Unités)
45
significant figures
(also, significant digits) all of the measured digits in a determination, including the uncertain last digit
46
solid
state of matter that is rigid, has a definite
shape, and has a fairly constant volume
47
symbolic domain
specialized language used to represent components of the macroscopic and microscopic domains, such as chemical symbols, chemical formulas, chemical equations, graphs, drawings, and calculations
48
temperature
intensive property representing the hotness or coldness of matter
49
theory
well-substantiated, comprehensive,
testable explanation of a particular aspect of nature
50
uncertainty
estimate of amount by which
measurement differs from true value
51
unit
standard of comparison for measurements
52
unit conversion factor
ratio of equivalent quantities expressed with different units; used to convert from one unit to a different unit
53
volume
amount of space occupied by an object
54
weight
force that gravity exerts on an object
55
Density formula
density = Mass/Volume (P = M/V)
56
Fahrenheit to Celsius
T°F = (9/5 × T°C) + 32
57
Celsius to Fahrenheit
T°C = 5/9 x (T°F-32)
58
Celsius to Kelvin
TK = °C + 273.15
59
Kelvin to Celsius
T°C = K - 273.15
60
Explain how you could experimentally determine whether the outside temperature is higher or lower than 0 °C (32 °F) without using a thermometer.
Place a bucket of water outside and observe it for some amount of time. If it freezes over, it is either 0 °C or colder. If the water still remains a liquid, then it must be warmer than 0 °C outside.
61
Identify each of the following statements as being most similar to a hypothesis, a law, or a theory. Explain your reasoning.
(a) Falling barometric pressure precedes the onset of bad weather.
(b) All life on earth has evolved from a common, primitive organism through the process of natural selection.
(c) My truck's gas mileage has dropped significantly, probably because it's due for a tune-up.
(a) Law, because it summarizes observations and applies them to the world in some way.
(b) Theory, because it is a well-substantiated explanation of nature.
(c) Hypothesis, because not only is it written in an "if-then" statement, but because it is a tentative observation of something of interest.
62
Identify each of the following statements as being most similar to a hypothesis, a law, or a theory. Explain your reasoning.
(a) The pressure of a sample of gas is directly proportional to the temperature of the gas.
(b) Matter consists of tiny particles that can combine in specific ratios to form substances with specific properties.
(c) At a higher temperature, solids (such as salt or sugar) will dissolve better in water.
(a) Law, because it states a consistently observed phenomenon that can be used for prediction.
(b) Theory, because it is a widely accepted explanation of the behavior of matter.
(c) Hypothesis, because it is a tentative explanation of something and can be investigated by experimentation.
63
Identify each of the underlined items as a part of either the macroscopic domain, the microscopic domain, or the symbolic domain of chemistry. For any in the symbolic domain, indicate whether they are symbols for a macroscopic or a microscopic feature.
(a) The mass of a **lead pipe** is 14 lb.
(b) The mass of a certain **chlorine atom** is 35 amu.
(c) A bottle with a label that reads **Al** contains aluminum metal.
(d) **Al** is the symbol for an aluminum atom.
(a) Macroscopic.
(b) Microscopic
(c) Symbolic, Macroscopic.
(d) Symbolic, Microscopic.
64
Identify each of the underlined items as a part of either the macroscopic domain, the microscopic domain,
or the symbolic domain of chemistry. For those in the symbolic domain, indicate whether they are symbols
for a macroscopic or a microscopic feature.
(a) A certain molecule contains one **H** atom and one Cl atom.
(b) **Copper wire** has a density of about 8 g/cm3.
(c) The bottle contains 15 grams of **Ni powder**.
(d) A **sulfur molecule** is composed of eight sulfur atoms.
(a) Symbolic, Microscopic.
(b) Macroscopic.
(c) Symbolic, Macroscopic.
(d) Microscopic.
65
According to one theory, the pressure of a gas increases as its volume decreases because the molecules in the gas have to move a shorter distance to hit the walls of the container. Does this theory follow a macroscopic or microscopic description of chemical behavior? Explain your answer.
Microscopic, because it calls for one to "imagine" this theory and gas molecules are described in a way that applies to the microscopic domain.
66
The amount of heat required to melt 2 lbs of ice is twice the amount of heat required to melt 1 lb of ice. Is this observation a macroscopic or microscopic description of chemical behavior? Explain your answer.
Macroscopic, because the heat required is determined from macroscopic properties.
67
Why do we use an object's mass, rather than its weight, to indicate the amount of matter it contains?
Weight is a factor of gravity (which can change depending on where something is located) and measuring by mass directly measures the amount of matter something contains regardless of where it is located.
68
What properties distinguish solids from liquids? Liquids from gases? Solids from gases?
Liquids can change their shape (flow); solids can't.
Gases can undergo large volume changes as pressure changes; liquids do not.
Gases flow and change volume; solids do not.
69
How does a heterogeneous mixture differ from a homogeneous mixture? How are they similar?
A heterogeneous mixture is a mixture with a composition that varies from point to point while a homogeneous mixture (solution) has a uniform composition throughout.
They both consist of two or more substances that are not chemically combined.
70
How does a homogeneous mixture differ from a pure substance? How are they similar?
The mixture can have a variety of compositions; a pure substance has a definite composition.
Both have the same composition from point to point.
71
The mixture can have a variety of compositions; a pure substance has a definite composition. Both have the same composition from point to point.
An element is a pure substance that cannot be broken down into a simpler substance while a compound is a pure substance that can be further broken down by chemical changes.
Both are forms of pure substances that have a constant composition.
72
How do molecules of elements and molecules of compounds differ? In what ways are they similar?
Molecules of elements contain only one type of atom; molecules of compounds contain two or more types of atoms.
They are similar in that both are comprised of two or more atoms chemically bonded together.
73
How does an atom differ from a molecule? In what ways are they similar?
An atom is the smallest particle of an element while a molecule is composed of two or more atoms themselves.
Both are similar in that they participate in chemical bonding and the formation of molecules and chemical formulas.
74
Many of the items you purchase are mixtures of pure compounds. Select three of these commercial products and prepare a list of the ingredients that are pure compounds.
Gatorade contains water, sugar, dextrose, citric acid, salt, sodium chloride, monopotassium phosphate, and sucrose acetate isobutyrate.
75
Classify each of the following as an element, a compound, or a mixture:
(a) copper
(b) water
(c) nitrogen
(d) sulfur
(e) air
(f) sucrose
(g) a substance composed of molecules each of which contains two iodine atoms
(h) gasoline
(a) Element
(b) Compound
(c) Element
(d) Element
(e) Mixture
(f) Compound
(g) Element
(h) Mixture
76
Classify each of the following as an element, a compound, or a mixture:
(a) iron
(b) oxygen
(c) mercury oxide
(d) pancake syrup
(e) carbon dioxide
(f) a substance composed of molecules each of which contains one hydrogen atom and one chlorine atom
(g) baking soda
(h) baking powder
(a) Element
(b) Element
(c) Compound
(d) Mixture
(e) Compound
(f) Compound
(g) Compound
(h) Mixture
77
A sulfur atom and a sulfur molecule are not identical. What is the difference?
Molecules and atoms are not the same things. A sulfur molecule is composed of eight sulfur atoms.
78
How are the molecules in oxygen gas, the molecules in hydrogen gas, and water molecules similar? How do they differ?
In each case, a molecule consists of two or more combined atoms.
They differ in that the types of atoms change from one substance to the next.
79
Why are astronauts in space said to be “weightless,” but not “massless”?
Anything that takes up space (an astronaut) and has mass contains matter. They can't be matter-less but can be weightless because they are not forced to the ground by a gravitational force.
80
Prepare a list of the principal chemicals consumed and produced during the operation of an automobile.
Gasoline (a mixture of compounds), oxygen, and to a lesser extent, nitrogen are consumed. Carbon dioxide and water are the principle products. Carbon monoxide and nitrogen oxides are produced in lesser amounts.
81
Matter is everywhere around us. Make a list by name of fifteen different kinds of matter that you encounter every day. Your list should include (and label at least one example of each) the following: a solid, a liquid, a gas, an element, a compound, a homogenous mixture, a heterogeneous mixture, and a pure substance.
Table, clothes, car, water, juice, milk, air, gas, oxygen, carbon dioxide, etc.
82
When elemental iron corrodes it combines with oxygen in the air to ultimately form red brown iron(III) oxide which we call rust.
(a) If a shiny iron nail with an initial mass of 23.2 g is weighed after being coated in a layer of rust, would you expect the mass to have increased, decreased, or remained the same? Explain.
(b) If the mass of the iron nail increases to 24.1 g, what mass of oxygen combined with the iron?
(a) Increased, because it would have combined with oxygen in the air thus increasing the amount of matter and therefore the mass.
(b) 0.9 g
83
As stated in the text, convincing examples that demonstrate the law of conservation of matter outside of the laboratory are few and far between. Indicate whether the mass would increase, decrease, or stay the same for the following scenarios where chemical reactions take place:
(a) Exactly one pound of bread dough is placed in a baking tin. The dough is cooked in an oven at 350 °F releasing a wonderful aroma of freshly baked bread during the cooking process. Is the mass of the baked loaf less than, greater than, or the same as the one pound of original dough? Explain.
(b) When magnesium burns in air a white flaky ash of magnesium oxide is produced. Is the mass of magnesium oxide less than, greater than, or the same as the original piece of magnesium? Explain.
(c) Antoine Lavoisier, the French scientist credited with first stating the law of conservation of matter, heated a mixture of tin and air in a sealed flask to produce tin oxide. Did the mass of the sealed flask and contents decrease, increase, or remain the same after the heating?
(a) No change.
(b) Decrease.
(c) No change.
84
Yeast converts glucose to ethanol and carbon dioxide during anaerobic fermentation as depicted in the simple chemical equation here: glucose ⟶ ethanol + carbon dioxide
(a) If 200.0 g of glucose is fully converted, what will be the total mass of ethanol and carbon dioxide produced?
(b) If the fermentation is carried out in an open container, would you expect the mass of the container and contents after fermentation to be less than, greater than, or the same as the mass of the container and contents before fermentation? Explain.
(c) If 97.7 g of carbon dioxide is produced, what mass of ethanol is produced?
(a) 200.0 g
(b) The mass of the container and contents would decrease as carbon dioxide is a gaseous product and would leave the container.
(c) 102.3 g
85
Classify the six underlined properties in the following paragraph as chemical or physical:
Fluorine is a pale yellow gas that reacts with most substances. The free element melts at −220 °C and boils
at −188 °C. Finely divided metals burn in fluorine with a bright flame. Nineteen grams of fluorine will
react with 1.0 gram of hydrogen.
Physical; chemical; physical; physical; chemical; chemical.
86
Classify each of the following changes as physical or chemical:
(a) condensation of steam
(b) burning of gasoline
(c) souring of milk
(d) dissolving of sugar in water
(e) melting of gold
Physical; chemical; chemical; physical; physical.
87
Classify each of the following changes as physical or chemical:
(a) coal burning
(b) ice melting
(c) mixing chocolate syrup with milk
(d) explosion of a firecracker
(e) magnetizing of a screwdriver
Chemical; physical; physical; chemical; physical.
88
The volume of a sample of oxygen gas changed from 10 mL to 11 mL as the temperature changed. Is this a chemical or physical change?
Physical change.
89
A 2.0-liter volume of hydrogen gas combined with 1.0 liter of oxygen gas to produce 2.0 liters of water vapor. Does oxygen undergo a chemical or physical change?
Chemical change.
90
Explain the difference between extensive properties and intensive properties.
The value of an extensive property depends on the amount of matter being considered, whereas the value of an intensive property is the same regardless of the amount of matter being considered.
91
Identify the following properties as either extensive or intensive.
(a) volume
(b) temperature
(c) humidity
(d) heat
(e) boiling point
(a) Extensive
(b) Intensive
(c) Extensive
(d) Extensive
(e) Intensive
92
The density (d) of a substance is an intensive property that is defined as the ratio of its mass (m) to its volume (V). density= mass/volume OR d= m/V
Considering that mass and volume are both extensive properties, explain why their ratio, density, is intensive.
Being extensive properties, both mass and volume are directly proportional to the amount of substance under study. Dividing one extensive property by another will in effect "cancel" this dependence on amount, yielding a ratio that is dependent of amount (an intensive property).
93
Is one liter about an ounce, a pint, a quart, or a gallon?
About a quart.
94
Is a meter about an inch, a foot, a yard, or a mile?
a yard
95
Indicate the SI base units or derived units that are appropriate for the following measurements:
(a) the length of a marathon race (26 miles 385 yards)
(b) the mass of an automobile
(c) the volume of a swimming pool
(d) the speed of an airplane
(e) the density of gold
(f) the area of a football field
(g) the maximum temperature at the South Pole on April 1, 1913
(a) Meters.
(b) Kilograms.
(c) Liters.
(d) Kilometers/hour.
(e) Grams/cubic centimeter.
(f) Square meters.
(g) Degrees Celcius.
96
Indicate the SI base units or derived units that are appropriate for the following measurements:
(a) the mass of the moon
(b) the distance from Dallas to Oklahoma City
(c) the speed of sound
(d) the density of air
(e) the temperature at which alcohol boils
(f) the area of the state of Delaware
(g) the volume of a flu shot or a measles vaccination
(a) Kilograms.
(b) Meters.
(c) Kilometers/second.
(d) Kilograms/cubic meter.
(e) Kelvin.
(f) Square meters.
(g) Cubic meters.
97
Give the name and symbol of the prefixes used with SI units to indicate multiplication by the following exact quantities.
(a) 10^3
(b) 10^−2
(c) 0.1
(d) 10^−3
(e) 1,000,000
(f) 0.000001
(a) Kilo (K), 10^3
(b) Centi (c), 10^-2
(c) Deci (d), 10^-1
(d) Milli (m), 10^-3
(e) Mega (M), 10^6
(f) Micro (μ), 10^-6
98
Give the name of the prefix and the quantity indicated by the following symbols that are used with SI base units.
(a) c
(b) d
(c) G
(d) k
(e) m
(f) n
(g) p
(h) T
(a) Centi, 10^-2
(b) Deci, 10^-1
(c) Giga, 10^9
(d) Kilo, 10^3
(e) Milli, 10^-3
(f) Nano, 10^-9
(g) Pico, 10^-12
(h) Tera, 10^12
99
A large piece of jewelry has a mass of 132.6 g. A graduated cylinder initially contains 48.6 mL water. When the jewelry is submerged in the graduated cylinder, the total volume increases to 61.2 mL.
(a) Determine the density of this piece of jewelry.
(b) Assuming that the jewelry is made from only one substance, what substance is it likely to be? Explain.
(a) 10.5 g/mL
(b) Silver, because it has the closest density to 10.5 g/mL.
100
Visit this density simulation (http://openstax.org/l/16phetmasvolden) and click the "turn fluid into water"
button to adjust the density of liquid in the beaker to 1.00 g/mL.
(a) Use the water displacement approach to measure the mass and volume of the unknown material
(select the green block with question marks).
(b) Use the measured mass and volume data from step (a) to calculate the density of the unknown
material.
(c) Link out to the link provided.
(d) Assuming this material is a copper-containing gemstone, identify its three most likely identities by
comparing the measured density to the values tabulated at this gemstone density guide
(https://www.ajsgem.com/articles/gemstone-density-definitive-guide.html).
(e) How are mass and density related for blocks of the same volume?
101
Visit this density simulation (http://openstax.org/l/16phetmasvolden) and click the "reset" button to
ensure all simulator parameters are at their default values.
(a) Use the water displacement approach to measure the mass and volume of the red block.
(b) Use the measured mass and volume data from step (a) to calculate the density of the red block.
(c) Use the vertical green slide control to adjust the fluid density to values well above, then well below, and
finally nearly equal to the density of the red block, reporting your observations.
102
Visit this density simulation (http://openstax.org/l/16phetmasvolden) and click the “turn fluid into water”
button to adjust the density of liquid in the beaker to 1.00 g/mL. Change the block material to foam, and
then wait patiently until the foam block stops bobbing up and down in the water.
(a) The foam block should be floating on the surface of the water (that is, only partially submerged). What
is the volume of water displaced?
(b) Use the water volume from part (a) and the density of water (1.00 g/mL) to calculate the mass of water
displaced.
(c) Remove and weigh the foam block. How does the block’s mass compare to the mass of displaced water
from part (b)?
103
Express each of the following numbers in scientific notation with correct significant figures:
(a) 711.0
(b) 0.239
(c) 90743
(d) 134.2
(e) 0.05499
(f) 10000.0
(g) 0.000000738592
(a) 7.11 * 10^2
(b) 2.39 * 10^-1
(c) 9.0743 * 10^4
(d) 1.342 * 10^2
(e) 5.499 * 10^-2
(f) 1.00000 * 10^4
(g) 7.38592 * 10^-7
104
Express each of the following numbers in exponential notation with correct significant figures:
(a) 704
(b) 0.03344
(c) 547.9
(d) 22086
(e) 1000.00
(f) 0.0000000651
(g) 0.007157
(a) 7.04 * 10^2
(b) 3.344 * 10^-2
(c) 5.479 * 10^2
(d) 2.2086 * 10^4
(e) 1.00000 * 10^3
(f) 6.51 * 10^-8
(g) 7.157 * 10^-3
105
Indicate whether each of the following can be determined exactly or must be measured with some degree of uncertainty:
(a) the number of eggs in a basket
(b) the mass of a dozen eggs
(c) the number of gallons of gasoline necessary to fill an automobile gas tank
(d) the number of cm in 2 m
(e) the mass of a textbook
(f) the time required to drive from San Francisco to Kansas City at an average speed of 53 mi/h
(a) Exact
(b) Measured
(c) Measured / Exact
(d) Exact
(e) Measured
(f) Measured
106
Indicate whether each of the following can be determined exactly or must be measured with some degree of uncertainty:
(a) the number of seconds in an hour
(b) the number of pages in this book
(c) the number of grams in your weight
(d) the number of grams in 3 kilograms
(e) the volume of water you drink in one day
(f) the distance from San Francisco to Kansas City
(a) Exact
(b) Exact
(c) Measured
(d) Exact
(e) Measured
(f) Measured
107
How many significant figures are contained in each of the following measurements?
(a) 38.7 g
(b) 2 x 10^18m
(c) 3,486,002 kg
(d) 9.74150 x 10^−4 J
(e) 0.0613 cm3
(f) 17.0 kg
(g) 0.01400 g/mL
(a) There are 3 significant figures.
(b) There are 1 significant figures.
(c) There are 7 significant figures.
(d) There are 6 significant figures.
(e) There are 3 significant figures.
(f) There are 3 significant figures.
(g) There are 4 significant figures.
108
How many significant figures are contained in each of the following measurements?
(a) 53 cm
(b) 2.05 x 10^8m
(c) 86,002 J
(d) 9.740 x 10^4 m/s
(e) 10.0613 m3
(f) 0.17 g/mL
(g) 0.88400 s
2, 3, 5, 4, 6, 2, and 5
109
The following quantities were reported on the labels of commercial products. Determine the number of
significant figures in each.
(a) 0.0055 g active ingredients
(b) 12 tablets
(c) 3% hydrogen peroxide
(d) 5.5 ounces
(e) 473 mL
(f) 1.75% bismuth
(g) 0.001% phosphoric acid
(h) 99.80% inert ingredients
a. 2
b. infinite
c. 1
d. 2
e. 3
f. 3
g. 1
h. 4
110
Round off each of the following numbers to two significant figures:
(a) 0.436
(b) 9.000
(c) 27.2
(d) 135
(e) 1.497 x 10^−3
(f) 0.445
a) 0.44
b) 9.0
c) 27
d) 140
e) 1.5 x 10^-3
f) 0.45
111
Round off each of the following numbers to two significant figures:
(a) 517
(b) 86.3
(c) 6.382 x 10^3
(d) 5.0008
(e) 22.497
(f) 0.885
(a) 520 (b) 86 (c) 6400 (d) 5.0 (e) 22 (f) 0.89
112
Deci
d : .1 : 10^-1
1 dL = 10^-1 L
1 L = 10dL
113
Centi
c = .01 = 10^-2
1cm = 10^-2
1m = 100cm
114
Milli
m = .001 = 10^-3
1ms = 10^-3
1s = 10^3 ms
115
Micro
u = .000001 = 10^-6
1ug = 10^-6
1g = 10^6 ug
116
Nano
n = .000000001 = 10^-9
1nm = 10^-9
1m = 10^9
117
Pico
p = .000000000001 =10^-12
1ps = 10^-12 s
1s = 10^12 ps
118
Femto
f = .000000000000001 = 10^-15
1fs = 10^-15s
1s = 10^15s
119
Mega
M = 1000000= 10^6
1Mg = 10^6 g
1g = 10^-6 Mg
120
Kilo
k = 1000 = 10^3
1km = 10^3 m
1m = 10^-3
121
1 inch
2.54 cm
122
1 meter
39.4 inches
123
1 kg
2.2 lbs
124
1lb
454 g
125
Conversion plan
126
A person’s average daily intake of glucose (a form of sugar) is 0.0833 pound (lb). What is this mass in milligrams (mg)?
(1 lb = 453.6 g.)
127
Alkali Metals
Group 1A ; Charge +1
128
Alkali Earth Metals
Group 2A ; Charge +2
129
Halogen
Group 7A/17 ; Charge -1
130
Noble Gases
Group 8A/18 : No charge
