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ILCC General Chemistry > Module 2: Atoms, Molecules, and Ions > Flashcards

Module 2: Atoms, Molecules, and Ions Flashcards

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1
Q

What is the atomic theory of matter?

A

The theory that atoms are the fundamental building blocks of matter

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2
Q

When did the atomic theory of matter emerge?

A

In the early 19th century

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3
Q

Who championed the atomic theory of matter?

A

John Dalton

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4
Q

What was John Dalton’s first postulate?

A

Each element is composed of extremely small particles called atoms

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5
Q

What was John Dalton’s second postulate?

A

All atoms of a given element are identical to one another in mass and other properties, but the atoms of one element are different from the atoms of all other elements

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6
Q

What was John Dalton’s third postulate?

A

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

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7
Q

What was John Dalton’s fourth postulate?

A

Atoms of more than 1 element combine to form compounds; a given compound always has the same relative number and kind of atoms

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8
Q

What is the law of conservation of mass?

A

The total mass of substances present at the end of a chemical process is the same as the mass of substances present before the process took place

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9
Q

The Law of Conservation of mass was one of the laws on which:

A

Dalton’s atomic theory was based

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10
Q

What is the law of multiple proportions?

A

IF 2 elements, A and B, form more than 1 compound, the masses of B that combine with a given mass of A are in the ratio of small whole numbers

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11
Q

What law did Dalton predict and observe while developing his atomic theory?

A

Law of multiple proportions

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12
Q

When 2 or more compounds exist from the same elements, they can not have:

A

The same relative number of atoms

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13
Q

In Dalton’s view, what was the smallest particle possible?

A

The atom

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14
Q

What is radioactivity?

A

The spontaneous emission of high-energy radiation by an atom

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15
Q

Who first observed radioactivity?

A

Henri Becquerel

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16
Q

Who also studied radioactivity?

A

Marie and Pierre Curie

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17
Q

What did the discovery of radioactivity show?

A

That an atom had more subatomic particles and energy associated with it

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18
Q

What 3 types of radiation were discovered by Ernest Rutherford?

A

alpha-particles (+ charge)
Beta-particles (- charge)
gamma-rays (uncharged)

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19
Q

What was the prevailing theory of the atom around 1900?

A

The “plum pudding” model (or chocolate chip cookie) that an atom was positive sphere of matter with negative electrons embedded in it

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20
Q

Who suggested the plum pudding model

A

JJ Thomson

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21
Q

What experiment did Ernest Rutherford do?

A

gold foil experiment

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22
Q

What was the gold foil experiment?

A

Rutherford shot alpha-particles at a thin sheet of gold foil and observed the pattern of scatter of the particles

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23
Q

What did Rutherford observe in his gold foil experiment?

A

Most alpha particles undergo no scattering, some particles are scattered and there is a wide variation in how far they scatter

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24
Q

What was the conclusion of the gold foil experiment?

A

Thomson’s plum pudding model of an atom could not be correct because some particles were deflected at large angles.
Since most particles did not deflect, conclusion that most of the atom is empty space
Since some particles are scattered, conclusion that there is a tiny positive nucleus in an atom

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25
Q

What did Rutherford postulate as a result of the gold foil experiment?

A

A very small, dense nucleus with electrons around the outside of the atom. Most of the atom is empty space.

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26
Q

How big is an atom

A

Hella small - 1-5 A or 100-500 pm

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27
Q

What are the (main) subatomic particles

A

Proton, neutron, electron

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28
Q

Charge of protons

A

+1

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29
Q

Charge of electrons

A

-1

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30
Q

Charge of neutrons

A

neutral

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31
Q

What (roughly) are the masses of the subatomic particles

A

Protons/neutrons are essentially the same mass (relative mass 1); mass of an electron is so small that we ignore it (relative mass 0)

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32
Q

Where are the subatomic particles located in an atom located

A

Protons and neutrons are in the nucleus, electrons travel around the nucleus

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33
Q

Actual mass of a proton

A

1.0073 amu

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34
Q

Actual mass of a neutron

A

1.0087 amu

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35
Q

Actual mass of an electron

A

5.486 x 10^-4 amu

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36
Q

What is the mass of the heaviest known atom?

A

4 x 10^-22 g

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37
Q

What is the scale for mass of atoms/ why is it different?

A

There is a different mass scale for atoms because they are so small (g are not a useful quantity). The atomic mass unit is the base unit (amu).

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38
Q

1 amu = how many grams?

A

1 amu = 1.66054 x 10^-24 g

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39
Q

How can atomic and molecular weight be measured very accurately?

A

With a mass spectrometer

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40
Q

Masses of atoms are compared to what?

A

A carbon atom with 6 protons and 6 neutrons (C-12)

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41
Q

Elements are represented by what?

A

A 1 or 2 letter symbol (Ex: carbon is C, hydrogen is H, neon is Ne)

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42
Q

What does the atomic number represent?

A

The number of protons in an atom

43
Q

What letter do we use for atomic number, and where is it written?

A

Z, written as a subscript before the symbol (subscript = bottom number)

44
Q

What does the mass number represent?

A

The total number of protons + neutrons in the nucleus of an atom

45
Q

Where do we write the mass number?

A

Superscript before the symbol (superscript = top number)

46
Q

What are isotopes?

A

Atoms of the same element with different masses

47
Q

Isotopes have the same number of ? but the same number of ?

A

Different number of neutrons, but same number of protons

48
Q

How many protons, electrons, and neutrons are in carbon-11, carbon-12, carbon-13, and carbon-14?

A

6 protons and 6 electrons in all isotopes. C-11 has 5 neutrons. C-12 has 6 neutrons. C-13 has 7 neutrons. C-14 has 8 neutrons.

49
Q

What is most of the carbon found in nature?

A

Almost 99% of the carbon found in nature is C-12

50
Q

Why do we use atomic weight in calculations?

A

Because we need to use very large amounts of atoms and molecules in the calculations

51
Q

How is average mass found?

A

Average mass is found using all isotopes of an element weighted by their relative abundances.

52
Q

Formula for atomic weight

A

Atomic weight = Sum of (isotope mass 1 x fractional natural abundance 1) + (isotope mass 2 x fractional natural abundance 2) …

53
Q

What is the periodic table

A

A systematic organization of all the elements

54
Q

How are elements arranged on the periodic table?

A

In order of atomic number

55
Q

What is the number at the top of a box for an element on the periodic table?

A

Atomic number

56
Q

What number do we write on the bottom of the box for an element on the periodic table?

A

atomic weight

57
Q

What are the rows called on the periodic table?

A

periods

58
Q

What are the columns called on the periodic table

A

Groups

59
Q

Elements of the same group share what?

A

similar chemical properties

60
Q

What does it mean that the periodic table has periodicity?

A

When one looks at the chemical properties of an element, one notices a repeating pattern of reactivities

61
Q

What 5 groups are known by special names on the periodic table?

A

1A, 2A, 6A, 7A, 8A

62
Q

What is the name for group 1A on the periodic table?

A

ALkali metals

63
Q

What elements are part of the alkali metals?

A

Li, Na, K, Rb, Cs, Fr

64
Q

What is the name for group 2A on the periodic table?

A

Alkaline earth metals

65
Q

What elements are part of the alkaline earth metals?

A

Be, Mg, Ca, Sr, Ba, Ra

66
Q

What is the name for group 6A on the periodic table?

A

Chalcogens

67
Q

What is the name for group 7A on the periodic table?

A

Halogens

68
Q

What is the name for group 8A on the periodic table?

A

Noble gases (or rare gases)

69
Q

What elements are part of the chalcogens?

A

O, S, Se, Te, Po

70
Q

What elements are part of the halogens on the periodic table?

A

F, Cl, Br, I, At

71
Q

What elements are part of the Noble gases on the periodic table?

A

He, Ne, Ar, Kr, Xe, Rn

72
Q

Where are metals located on the periodic table?

A

Left side

73
Q

What are some properties of metals?

A

Shiny luster, good conductors of heat and electricity, solid at room temperature (except mercury)

74
Q

Where are nonmetals located on the periodic table

A

Right side (except H is also a nonmetal) (top right corner)

75
Q

What states can nonmetals be at room temp

A

Solid (like carbon), liquid (like bromine), or gas (like neon)

76
Q

What is the line that divides metals and nonmetals called

A

Steplike line

77
Q

What type of elements are found along the steplike line?

A

Metalloids

78
Q

What elements are metalloid?

A

B, Si, Ge, As, Sb, Te, (maybe also element number 117. science isn’t really sure yet)

79
Q

What are the elements along the steplike line that are not considered metalloids?

A

Al, At, Po (Po is debatable apparently)

80
Q

What are the properties of metalloids?

A

Sometimes like metals and sometimes like nonmetals

81
Q

In a chemical formula, what does the subscript to the right of an element’s symbol tell?

A

The number of atoms of that element in 1 molecule of that compound

82
Q

What are molecular compounds usually composed of?

A

Usually only nonmetals

83
Q

What is a diatomic molecule?

A

A molecule that only contains 2 atoms of the same element

84
Q

What are the 7 naturally occurring diatomic molecules?

A

H2, N2, O2, F2, Cl2, Br2, I2

85
Q

What elements form diatomic molecules in nature?

A

hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, iodine

86
Q

List 4 types of formulas

A

Empirical formulas, molecular formulas, structural formulas, perspective drawings

87
Q

What is an empirical formula?

A

Formula that gives the lowest whole-number ratio of atoms of each element in a compound

88
Q

What is a molecular formula?

A

Formula that gives the exact number of atoms of each element in a compound

89
Q

If we know the molecular formula, what other formula can we determine?

A

The empirical formula

*The reverse is NOT TRUE!

90
Q

What is a structural formula?

A

Formula that shows the order in which atoms are attached. They DO NOT depict the 3D shapes of molecules

91
Q

What is a perspective drawing?

A

Drawing that shows the 3D order of the atoms in a compound. Also demonstrated using models

92
Q

What is it called when an atom gains or loses an electron?

A

It becomes an ion

93
Q

When does a cation form?

A

When at least 1 electron is lost

94
Q

What type of elements form monatomic cations?

A

metals

95
Q

Define cation

A

positively charged ion

96
Q

define anion

A

negatively charged ion

97
Q

When does an anion form

A

when at least 1 electron is gained

98
Q

What type of element forms monatomic anions

A

nonmetals

99
Q

What types of elements usually form an ionic compound?

A

Metals and nonmetals

100
Q

What structure do ionic compounds usually form?

A

Crystalline structures

101
Q

How do ionic compounds form

A

Electrons are transferred from the metal to the nonmetal. The oppositely charged ions attract each other

102
Q

What type of formula do we write for ionic compounds

A

Only empirical formulas

103
Q

Because compounds are electrically neutral, describe how one can determine the formula of a compound

A

The charge of the cation becomes the subscript of the anion.
The charge on the anion becomes the subscript on the cation.
If these subscripts are not the lowest whole-number ratio, divide them by the greatest common factor

ILCC General Chemistry (2 decks)

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