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Year 1 Chemistry > 1.1 Atomic Structure > Flashcards

1.1 Atomic Structure Flashcards

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1
Q

All elements are made up of…

A

Atoms

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2
Q

3 types of sub-atomic particle and their charges.

A

Protons +1
Electrons -1
Neutrons 0

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3
Q

Most of the mass of an atom is concentrated in the….

A

Nucleus

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4
Q

Mass number

A

The total number of protons and neutrons in the nucleus of an atom.

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5
Q

Atomic (proton) number

A

The number of protons in the nucleus of an atoms.

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6
Q

All atoms of the same element have the same number of….

A

protons

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7
Q

Atoms form ions by….

A

Gaining or losing electrons.

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8
Q

What is an isotope?

A

Atoms with the same number of proton but a different number of neutrons.

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9
Q

What is Dalton’s model

A

Atoms are solid spheres and different spheres make up different elements

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10
Q

What is Thomson’s model?

A

Atoms were a large positively charged ‘pudding’ with electrons stuck on them.

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11
Q

What is Rutherford’s model?

A

A tiny positively charged nucleus surrounded by a cloud of negative electrons. Most of the atom is empty space.

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12
Q

What is Bohr’s model?

A

Electrons exist in fixed orbits or shells.
Each shell has a fixed energy.
When an electron moves between shell radiation is absorbed or emitted.
The radiation will have a fixed frequency.

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13
Q

What is Ar

A

Relative atomic mass - the average mass of an element on a scale where carbon 12 is exactly 12

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14
Q

What is relative isotopic mass

A

The mass of an atom of an isotope on a scale where carbon 12 is exactly 12

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15
Q

What is Mr

A

Relative molecular mass - the average mass of a molecule on a scale where carbon 12 is exactly 12.

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16
Q

How do you find the Mr of a molecule.

A

Add up all the Ar values for all the elements in the molecule

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17
Q

Calculate the Mr of C2H6O

A

(2x12.0) + (6x1.0) + (1x16.0) = 46.0

18
Q

What is relative formula mass

A

The average mass of a formula unit on a scale where an atom of carbon 12 is exactly 12

19
Q

Calculate the relative formula mass od CaF2

A

40.1 + (2x19.0) = 78.1

20
Q

Describe how a mass spectrometer works.

A

Ionisation - Sample is dissolved in a polar solvent and pushed through a nozzel at high pressure with a high voltage applied causing the particles to lose an electron.
Acceleration - Positive ions are accelerated by an electric field. Ions with a lower masses are accelerated more than heavier ones
Ion drift - Ions enter a region with non electric field. Those which are heavier drift slower
Detection - Ions hit a detector plate where they gain an electron producing a current. The strength of this current shows relative abundance.

21
Q

The further a shell is from the nucleus…

A

the higher it energy level

22
Q

Shells are divided up into

A

Sub-shells

23
Q

What are the names of each sub-shell

A

s,p,d,f

24
Q

What are orbitals

A

Regions where there is a 95% chance of finding an electron. Each orbital can contain up to 2 electrons.

25
Q

How many electrons can the s level hold?

A

2

26
Q

How many electrons can the p level hold?

A

6

27
Q

How many electrons can the d level hold?

A

10

28
Q

How many electrons can the f level hold?

A

14

29
Q

What sub-shells does the 1st shell contain?

A

s

30
Q

What sub-shells does the 2nd shell contain?

A

s,p

31
Q

What sub-shells does the 3rd shell contain?

A

s,p,d

32
Q

What sub-shells does the 4th shell contain?

A

s,p,d,f

33
Q

Electron configuration rules

A

1) electrons fill up the lowest energy level first
2) electrons fill orbitals in a sub-shell singly before they start sharing
3) for ions in the s and p blocks add or remove electrons from the highest occupied energy level

34
Q

What do copper and chromium do?

A

They donate one of their 4s electrons to the 3d sub shell

35
Q

Full configuration of copper

A

1s2 2s2 2p6 3s2 3p6 3d10 4s1

36
Q

What is the s block

A

Group 1 and 2 elements

37
Q

What is the p block

A

group 5,6 and 7 elements

38
Q

What is the d block

A

Transition metals

39
Q

What is first ionisation energy

A

The energy required to remove 1 electron from each atom in one mole of gaseous atoms to from 1 mole of gaseous 1+ ions

40
Q

What does it mean if there is a high first ionisation energy

A

There is high attraction between the electron and the nucleus.

41
Q

Factor affect first ionisation energy.

A

Nuclear charge - more protons increase that charge in the nucleus which increases attraction
Distance from nucleus - Attraction decreases as distance increases
Shielding - As the number of electrons between the outermost electron and nucleus increases the attraction decreases

Year 1 Chemistry (12 decks)

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