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Inorganic Chemistry > M2-L1: Early Concepts About the Atom > Flashcards

M2-L1: Early Concepts About the Atom Flashcards

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1
Q

All matter is composed of minute, sub microscopic, indivisible particles called _____.

A

Atoms

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2
Q

The earliest model of the atom was developed by the ancient _____ philosophers and Scientists in the past.

A

Greek

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3
Q

The discoveries of the modern scientist disproved ______’s theory.

A

John Dalton

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4
Q

There are many kinds of atoms as there are kinds of elements, which are chemically _________ from each other.

A

Different

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5
Q

Isotopes are atoms of the same element having different ______ ____.

A

Atomic Mass

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6
Q

An ____ is composed of a tiny core or nucleus with electrons outside the nucleus.

A

Atom

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7
Q

An atom is composed of a tiny core or _______ with electrons outside the nucleus.

A

Nucleus

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8
Q

An atom is composed of a tiny core or nucleus with _________ outside the nucleus.

A

Electrons

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9
Q

The nucleus contains protons but no ________.

A

Electrons

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10
Q

The negative charge on the electrons balances the positive charge on the nucleus so that an atom is electrically ______.

A

Neutral

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11
Q

At least 99.9% of the mass of an atom is in the _______.

A

Nucleus

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12
Q

The electrons are at relatively large distances from the _______.

A

Nucleus

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13
Q

An atom is mostly empty _____.

A

Space

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14
Q

The small, dense center of positive charge in the atoms.

A

Nucleus

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15
Q

Uncharged particle.

A

Neutron

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16
Q

The sum of masses of proton and neutron.

A

Atomic Mass

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17
Q

Element with the same atomic number but different atomic mass.

A

Isotopes

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18
Q

Sublevel s has how many maximum number of electrons?

A

2

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19
Q

Sublevel p has how many maximum number of electrons?

A

6

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20
Q

Sublevel d has how many maximum number of electrons?

A

10

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21
Q

Sublevel f has how many maximum number of electrons?

A

14

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22
Q

Each orbitals have a maximum of ___ electrons.

A

Two

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23
Q

Modifications of the Bohr’s theory led to the theory of atomic structure which is based on _______ mechanics or wave mechanics.

A

Quantum

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24
Q

This theory shows that electrons tend to occupy various energy levels designated as K,L,M,N,O etc. or 1,2,3,4, etc.

A

Schrodinger’s Wave Mechanical Model of the Atom

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25
Q

Shells 1, 2, 3, and 4 corresponds to what shell letters?

A

1 = K
2 = L
3 = M
4 = N

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26
Q

Shell K or 1 has _ maximum number of electrons.

A

2

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27
Q

Shell L or 2 has _ maximum number of electrons.

A

8

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28
Q

Shell M or 3 has _ maximum number of electrons.

A

18

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29
Q

Shell N or 4 has _ maximum number of electrons.

A

32

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30
Q

Proposed a model of the atom in terms of waves.

A

Quantum Theory or Waves Theory (Erwin Schrodinger)

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31
Q

Paved the way for the development of the wave mechanics.

A

Heisenberg’s Theory

32
Q

This theory states that the exact position and exact location of the electron cannot be pinpointed.

A

Heisenberg’s Theory

33
Q

In the wave mechanical model, the electron can be determined only in terms of _______.

A

Orbital

34
Q

The energy state of the electron in an atom can be described by a set of numbers called the quantum numbers _, _, _, _,.

A

n, l, m, s

35
Q

Set the probability within which an electron can be found.

A

Four quantum numbers

36
Q

Describes the relative position of these energy level, their distance from nucleus and the energy of an electron.

A

Principal quantum number (n)

37
Q

Principal Quantum numbers are represented by numbers 1,2,3,4 . . . or letters _, _, _, _.

A

K, L, M, N

38
Q

Describes the shape of the orbital on the electron cloud.

A

Azimuthal/Subsidiary/Orbital quantum number

39
Q

AQN (l): Is represented by what letters?

A

s, p, d, f

40
Q

AQN (l): The value of s is?

A

0

41
Q

AQN (l): The value of p is?

A

1

42
Q

AQN (l): The value of d is?

A

2

43
Q

AQN (l): The value of f is?

A

3

44
Q

Describes the spatial orientation of the orbitals.

A

Magnetic quantum number

45
Q

It is dependent on the values of azimuthal quantum number.

A

Magnetic quantum number

46
Q

This number describes the direction the electron is spinning in a magnetic field — either clockwise or counterclockwise.

A

Spin quantum number

47
Q

The first person to come up with an idea of an atom.

A

Democritus

48
Q

He used the word “atomos”, which is a Greek word for uncuttable or smallest indivisible and indestructible particle.

A

Democritus

49
Q

He did not believe that matter is made up of tiny particles called atoms.

A

Aristotle

50
Q

He believed that matter is made out of five elements: earth, water, air, fire, and aether.

A

Aristotle

51
Q

He studies how gases combine, react, and move with temperature and pressure.

A

John Dalton

52
Q

He developed his idea called the “atomic theory.”

A

John Dalton

53
Q

He discovered that atoms could be divided, and discovered the negatively charged particle called the “electron.”

A

JJ Thompson

54
Q

He called his theory the “plum pudding model⁠.”

A

JJ Thompson

55
Q

He is responsible for the discovery of protons.

A

William Goldstein

56
Q

He fired alpha particles at a very thin sheet of gold foil.

A

Ernest Rutherford

57
Q

He discovered that the atom contained a dense center which was positively charged/had the proton.

A

Ernest Rutherford

58
Q

He discovered that the atom was made up of mostly empty space.

A

Ernest Rutherford

59
Q

His model is called the “Bohr Model of the Atom.”

A

Niels Bohr

60
Q

He found that electrons will actually travel around the atom in discrete energy levels; that electrons can never exist between energy levels.

A

Niels Bohr

61
Q

He also found that electrons can move up an energy level if they are given enough energy.

A

Niels Bohr

62
Q

He called this amount of energy as a “quantum of energy.” 

A

Niels Bohr

63
Q

He proposed that waves can act like particles, and particles can act like waves.

A

Louis De Broglie

64
Q

He suggested that electrons can better be described as waves rather than as particles.

A

Louis De Broglie

65
Q

He proposed that one of the implication of electrons behaving like waves is that you cannot know both the speed and position of an electron at the same time.

A

Werner Heisenberg

66
Q

He developed a mathematical equation to show where the electrons are located around the nucleus.

A

Erwin Schrodinger

67
Q

He showed us that with his wave equation that we can only know regions of probability of finding an electron, which is called the “electron cloud model.”

A

Erwin Schrodinger

68
Q

Erwin Schrodinger showed us that with his wave equation that we can only know regions of probability of finding an electron, which is called the “________ _____ _____.”

A

Electron Cloud Model

69
Q

He was responsible for the discovery of the neutron.

A

James Chadwick

70
Q

Identical to electron but with a positive charge.

A

Position

71
Q

Uncharged species of zero mass.

A

Neutrino

72
Q

An electron unstable particle omitted from the nucleus.

A

Betatron

73
Q

Principle: Electrons tend to occupy a lower orbital surface going to a higher energy orbital.

A

Aufbau Principle or Building up principle

74
Q

Principle: The maximum number of electrons in an orbital is two and they must be of opposite spin.

A

Paulis Exclusion Principle

75
Q

When a number of degenerate orbitals are available and there is no electron to fill up, all other orbitals to full capacity of two electrons, each member of the degenerate set receives one electron, before anyone of the set receives two electrons.

A

Hund’s Rule

Inorganic Chemistry (9 decks)

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