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Chemistry 4U > Unt 1 - Atomic Structure > Flashcards

Unt 1 - Atomic Structure Flashcards

1
Q

What year did Dalton create the Billard ball model?

A

1809

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2
Q

What was the limitation of Dalton’s Billard ball model

A

It could not explain why atoms of elements combine in the way they do

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3
Q

What was Thompson’s model and what year was it created

A

1887,
A chocolate chip cookie
Electrons in a positive sphere

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4
Q

Why was Thompson’s model better than Dalton’s?

A

He discovered the electron and charges which explained why atoms combine in their ratios

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5
Q

What and who disproved Thompson’?

A

Rutherford with the gold foil experiment

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6
Q

What year was Rutherford’s diagram created and what did it look like?

A

1909
Positive nucleus, electrons floating around

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7
Q

What were the limitations on Rutherford’s theory?

A

-A nucleus of only positive charges would repel
- didn’t account for entire weight of an atom
- Electrons in motion should continuously give off radiation (light) and lose energy, atoms would implode

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8
Q

What did Bohr’s diagram look like and what year was it created?

A

1913,
Orbits of electrons and energy levels

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9
Q

Limitations of Bohr diagram

A

-Could only explain single electron atoms (H, He, Li etc)

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10
Q

Why did Bohr disprove Rutherford?

A

Energy emitted should be continuous but it is not
Within energy level electrons do not emit energy
Electrons change level by absorbing or emitting energy

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11
Q

Who discovered neutrons?

A

James Chadwick, 1932

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12
Q

Who discovered protons?

A

Rutherford, 1914

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13
Q

Who discovered isotopes?

A

Frederick Soddy, 1913

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14
Q

What is a photon?

A

A particle of light
What a quantum of light energy is called

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15
Q

What is a Quantum?

A

A packet of energy
Plank

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16
Q

What is a continuous spectrum?

A

The spectrum that consists of a continuum of wavelengths

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17
Q

What is Emission spectrum?

A

The spectrum of frequencies of electromagnetic radiation emitted due to an electron making a transition from high energy state to a lower energy state

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18
Q

What is an absorption spectrum?

A

The spectrum of frequencies of electromagnetic radiation absorbed due to an electron making a transition from a low energy state to a higher energy state

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19
Q

In an orbit, are electrons a fixed or variable difference from the nucleus?

A

Fixed distance

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20
Q

Are orbitals 2D or 3D?

A

3D

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21
Q

How many electrons are there per orbital?

A

2

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22
Q

How many electrons in an orbit?

A

2, 8 or 18

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23
Q

An orbital with 1 orbital orientation, up to 2 electrons that is in all energy levels is called…

A

S-shape

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24
Q

An orbital with 3 orbital orientations, up to 6 electrons that is in energy level 2 and up is called…

A

P-shape

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25
Q

An orbital with 5 orbital orientations, up to 10 electrons and in energy level 3 and up is called…

A

D-shape

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26
Q

An orbital with 7 orbital orientations, up to 14 electrons and is in energy level 4 and up is called…

A

F-shape

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27
Q

What is the right order when writing an energy level diagram?

A

1s, 2s, 2p, 3s, 3p, 4s, 4d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 5f, 6d

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28
Q

What can the row an element is in on the periodic table tell you about its energy level diagram?

A

Energy level

29
Q

What can the row an element is in on the periodic table tell you about its energy level diagram?

A

Energy level

30
Q

What form of diagram/ configuration do you draw the direction of spin each electron has?

A

Energy level diagram

31
Q

What is this an example of?

1s^2, 2s^2, 2p^6, 3s^2, 3p^1

A

Complete electron configuration

32
Q

What is this an example of?
[Ne] 3s^2, 3p^1

A

Condensed electron configuration

33
Q

What does VSEPR stand for?

A

Valence Shell Electron Pairs Repel

34
Q

What is VSEPR theory?

A

Pairs of electrons in valence shell stay as far away as possible

35
Q

What is a Hybrid orbital?

A

Atomic orbitals overlap to form new orbital containing a pair of electrons of opposite spin

36
Q

Which VSPER shapes are always non-polar?

A

Linear
Linear
Trigonal Planar
Tetrahedral

37
Q

What VSEPR shapes may be polar?

A

Bent/Angular
Bent/Angular
Pyramidal

38
Q

What EN difference does a bond need to be polar?

A

0.4-1.8

39
Q

What EN difference does a bond need to be polar?

A

0.4-1.8

40
Q

EN difference of a covalent bond?

A

<0.4

41
Q

EN difference of an ionic bond

A

> 1.8

42
Q

EN difference of an ionic bond

A

> 1.8

43
Q

Give 2examples if intramolecular forces

A

Ionic and Covalent

44
Q

What is an intramolecular force?

A

Forces between atoms and ions within a molecule

45
Q

Which is stronger, intermolecular forces or intramolecular forces?

A

Intramolecular

46
Q

What is another name for intermolecular forces?

A

Van def Waals forces

47
Q

What is an intermolecular force?

A

Attractive forces between molecules

48
Q

What are weaker, intermolecular forces or intramolecular forces?

A

Intermolecular forces

49
Q

What are 3 examples of intermolecular forces?

A

H-bonds, dipole-dipole, London dispersion forces

50
Q

Does it take less energy to melt a substance or break it down into separate elements?

A

Melt a substance

51
Q

What is a dipole-dipole force

A

Attraction between oppositely charged ends of polar molecules

52
Q

Which intermolecular force is the weakest?

A

London dispersion

53
Q

What is a London dispersion force?

A

Nucleus attracts electrons from neighbouring molecules
Present in all molecules, important in non-polar molecules
At moderate distance attraction can be stronger than the repulsion of electrons

54
Q

The higher amount of electrons the ________ the London force

A

Stronger

55
Q

The _________ amount of electrons the weaker the London force

A

Lower

56
Q

What size of molecules have low boiling points

A

Small neutral molecules

57
Q

Do big molecules have high or low boiling points?

A

High

58
Q

Molecules with the approximate same London forces have the same amount of _______

A

Electrons

59
Q

The more polar a molecule and the stronger the dipole-dipole attraction the ___________

A

Higher the boiling point

60
Q

What is the strongest intermolecular force?

A

Hydrogen bonds

61
Q

What is a hydrogen bond?

A

Strong dipole-dipole force

62
Q

H-bonds are _____%-______% as strong as covalent bonds

A

5%-10%

63
Q

What elements does hydrogen bond with in H-bonds?

A

Fluorine
Oxygen
Nitrogen

64
Q

Rank the intermolecular forces from weakest to strongest

A

London dispersion
Dipole-dipole
H-bonds

65
Q

The higher the force the higher the __________+__________

A

Melting point and boiling point

66
Q

What is an ion dipole?

A

Ion and polar molecule
Ex. NaCl separating into ions when surrounded by water

67
Q

Ion induced dipole,
Ex O2 sticks to hemoglobin in bloodstream

A

Ion close to non polar molecule induced temp dipole

68
Q

Dipole induced dipole

A

Chemistry 4U (1 decks)

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