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Inorganic and Organic Chemistry (Lecture) > Module 2 ( Atomic Theory, Electron Configuration, The Quantum Mechanical Model, The Periodic Table) > Flashcards

Module 2 ( Atomic Theory, Electron Configuration, The Quantum Mechanical Model, The Periodic Table) Flashcards

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1
Q

The scientific description of nature of atoms

A

Atomic Theory

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2
Q

He came up with the idea that if you continued to cut something, eventually you would end up with something that couldn’t be cut anymore

A

Democritus

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3
Q

What is an atom?

A

The smallest particle that an element can be divided and still be the same substance

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4
Q

Atomos means?

A

cannot be divided

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5
Q

He realized that atoms combine in very specific proportions based on mass

A

John Dalton (1803)

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6
Q

John Dalton’s model

A

Solid Sphere Model

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7
Q

On what model indicated that all substances are made of atoms that cannot be created, divided, or destroyed

A

Dalton’s Solid Sphere Model

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8
Q

Who was the proponent of the Plum Pudding Model and when was it proposed?

A

J.J Thompson (1897)

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9
Q

What does the plum pudding model indicate?

A

Electrons are mixed throughout the atom, like a soup or a plum pudding

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10
Q

Who discovered electrons?

A

J.J Thompson

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11
Q

What did Ernest Rutherford discover in 1909?

A

He discovered that an atom contains a nucleus with positively charged particles and electrons must be floating around the nucleus

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12
Q

True or False. Rutherford indicates that most of an atom is empty space

(If false, correct the statement)

A

True

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13
Q

He proposed that electrons move around the nucleus in energy levels but no electrons in between

A

Niels Bohr (1913)

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14
Q

True or False. According to Bohr, electrons have a tendency to stay only on their corresponding energy levels.

(If false, correct the statement)

A

False.

Electrons can jump from one level to another.

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15
Q

Who were the proponents of the Modern Atomic Theory?

A

Erwin Shrodinger and Werner Heisenberg

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16
Q

Modern Atomic Theory indicates that…

A

Electrons have no predictable pattern and move in a region called the electron cloud.

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17
Q

What does it mean when:

a) protons = electrons
b) protons > electrons
c) protons < electrons

A

a) an atom has no charge
b) has positive charge
c) has a negative charge

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18
Q

Electrons, protons, and neutrons are called?

A

Subatomic particles

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19
Q

True or False. Bohr found that “cathode rays” were actually particles travelling from cathode to anode and called them electrons

(If false, correct the statement)

A

False.

Thompson found that “cathode rays” were actually particles traveling from cathode to anode and called them electrons.

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20
Q

Who discovered neutrons?

A

James Chadwick (1932)

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21
Q

What charges can be found in the nucleus? Outside the nucleus?

A

Protons and neutrons in the nucleus.

Electrons are surrounding the nucleus.

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22
Q

It is the number of protons which is also the number of electrons

A

Atomic number

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23
Q

True or False. The atomic number is unique to each element.

If false, correct the statement

A

True

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24
Q

What is the mass number?

A

The sum of protons and neutrons

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25
Q

Enumerate the three nuclei of H isotopes

A

Protium, Deuterium, and Tritium

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26
Q

It describes how the electrons are distributed in the various atomic orbitals.

A

Electron configuration

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27
Q

What are the two ways of writing electron configuration

A

spdf notation, orbital box notation

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28
Q

It states that electrons enter the lowest energy orbitals first.

A

Aufbau’s Principle

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29
Q

True or False. If the principal quantum number (n) is lower, then the energy level is higher.

(If false, correct the statement)

A

False.

The lower the n, the lower the energy.

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30
Q

An atomic orbital may only have up to 2 electrons.

A

Pauli’s Exclusion Principle

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31
Q

Explain Hund’s rule.

A

It states that in degenerating orbitals, you fill half way first before pairing electrons.

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32
Q

Degenerate orbital means…

A

they have the same energy

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33
Q

True or False. A similar configuration causes them to behave chemically

(If false, correct the statement)

A

True

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34
Q

The total number of electrons that can be accommodated in an energy level.

A

2n^2

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35
Q

The principal quantum number is also known as…

A

Bohr’s spectral lines

36
Q

Splitting of Bohr’s spectral lines under a high-resolution spectroscope

A

Azimuthal quantum number

37
Q

The azimuthal is also known as…

A

sub energy levels or orbitals

38
Q

Values of azimuthal quantum #

A

0 to n-1

39
Q

Indicate the energy level when l = 0, 1, 2, 3

A

0 - s orbital
1 - p orbital
2 - d orbital
3 - f orbital

40
Q

Splitting of high-resolution lines in a magnetic field

A

Magnetic quantum number

41
Q

True or False. The magnetic quantum number is also called angular momentum.

(If false, correct the statement)

A

True

42
Q

Values of the magnetic quantum number range from

A

-l to 0 +l

43
Q

Spin Quantum Number

A

Indicates electron spin in the orbital

44
Q

Values for the spin quantum number

A

-1/2, +1/2

45
Q

The area around the nucleus where the probability of finding the electrons are maximum.

A

Orbitals

46
Q

Indicate the shapes of each orbital.

A

s - sphere-shaped
p - dumbbell-shaped
d - double dumbbell-shaped
f - lobbed dumbbell

47
Q

How many electrons can each orbital hold?

A

s - 2
p - 6
d - 10
f - 14

48
Q

Who introduced the 4 initial elements and what are those?

A

Aristotle

Fire, Water, Air, Earth

49
Q

This is when 14 elements were known

A

1700

50
Q

He wrote the first extensive list of 33 elements.

A

Antoine Lavoisier

51
Q

What did Johann Dobereiner found out in 1829?

A

In a group of three, the average atomic mass of the first and third elements is equal to the atomic mass of the second element.

52
Q

Who formulated the Law of Triads?

A

Johann Dobereiner

53
Q

He arranged the known 62 elements from lightest to heaviest based on increasing atomic weights

A

John Newlands (1864)

54
Q

True or False. Mendeleev noticed that every 8th element had similar chemical and physical properties.

(If false, correct the statement)

A

False.

Newlands noticed that every 8th element had similar chemical and physical properties.

55
Q

Who is the proponent of the Law of Octaves?

A

John Newlands

56
Q

A Russian chemist that organized elements by their atomic mass.

A

Dmitri Mendeleev (1869)

57
Q

The Father of Modern Periodic Table

A

Dmitri Mendeleev

58
Q

It states that the physical and chemical properties of elements are periodic functions of their atomic weights.

A

Periodic Law

59
Q

He arranged elements by atomic number

A

Henry Moseley

60
Q

Properties of elements are periodic functions of their atomic number

A

New Periodic Law

61
Q

He helped establish noble gases as a new group in the periodic table.

A

William Ramsay (1904)

62
Q

What did Ramsay discovered and which is the first?

A

Noble gases.

Helium and Argon are the first to be discovered.

63
Q

He discovered 8 new elements and the only living person whom an element was named.

A

Glenn Seaborg

64
Q

How many elements are there?

A

118 elements, 82 naturally occurred on Earth, 36 have been created

65
Q

Indicate which are period and group in a periodic table.

A

Period/ series - horizontal rows

Group/ Family - vertical columns

66
Q

Where are metals, metalloids, and nonmetals located in the periodic table?

A

Metal - left side
Nonmetals - right side
Metalloid - boundary

67
Q

The most metallic element

A

Francium (Fr)

68
Q

It has the tendency to lose electrons and form cations.

A

Metals

69
Q

Good insulators and has a tendency to gain electrons and form anions.

A

Nonmetals

70
Q

The most reactive nonmetal

A

Fluorine

71
Q

Elements have similar properties due to the similarities in the number of electrons in outer shells

A

The Group

72
Q

Two categories of group/family

A

Group A - Representative elements

Group B - Transition Elements

73
Q

Horizontal rows are also known as series.

A

Period

74
Q

True or False. n is the same as the periodic number.

If false, correct the statement

A

True

75
Q

It states that atoms or ions often react to obtain exactly eight electrons in their valence shell.

A

Octet rule

76
Q

Group 1A and very reactive in its elemental form.

A

Alkali Metals

77
Q

They form compounds with halogens similar to table salt.

A

Alkali Metals

78
Q

A very reactive group of elements.

A

Halogens

79
Q

What are noble gases?

A

Group 8 of elements that are very stable and are unreactive gases.

80
Q

It is half the distance between the nuclei of 2 like atoms.

A

Atomic Radius

81
Q

True or False. As you move down the group, the atomic radius decreases. And as you move across, it increases.

(If false, correct the statement)

A

False.

As you move down, it increases. It decreases as it moves from left to right.

82
Q

What is ionization energy?

A

The energy required to remove 1 electron from an atom.

83
Q

What does it mean when there is low ionization? high ionization?

A

Low IE - easy to remove the electrons

High IE - hard to remove electrons

84
Q

True or False. As you move down, ionization decreases. It increases as you move across from left to right,
(If false, correct the statement)

A

True.

85
Q

True or False. As you move down, electronegativity decreases. It increases as you move across from left to right,
(If false, correct the statement)

A

True

86
Q

The tendency of an element to be shiny, silver, and malleable,

A

Metallic character

87
Q

True or False. As you move down, the metallic character decreases. It increases as you move across from left to right,
(If false, correct the statement)

A

False.

As you move down, the metallic character increases. It decreases as you move across from left to right.

Inorganic and Organic Chemistry (Lecture) (6 decks)

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