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AS Chemistry Module 1 > 1.2 - Atomic Structure > Flashcards

1.2 - Atomic Structure Flashcards

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1
Q

What is the relative mass of an electron?

A

1/1837

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2
Q

Where are electrons found in atoms?

A

The shells of atoms

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3
Q

Atomic number definition

A

The number of protons in the nucleus of an atom.

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4
Q

Mass number definition

A

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

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5
Q

Relative Atomic Mass (RAM) definition

A

The average (weighted mean) mass of an atom of an element relative to one-twelfth of the mass of an atom of carbon-12.

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6
Q

Relative Isotopic Mass (RIM) definition

A

The mass of an atom of an isotope of an element relative to one-twelfth of the mass of an atom of carbon-12.

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7
Q

Isotopes definition

A

Atoms which have the same atomic number but a different mass number (contain the same number of protons but different number of neutrons).

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8
Q

Relative Molecular Mass (RMM) definition

A

The average (weighted mean) mass of a molecule relative to one-twelfth of the mass of an atom of carbon-12.

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9
Q

Relative Formula Mass (RFM) definition

A

The average (weighted mean) mass of a formula unit relative to one-twelfth of an atom of carbon-12.

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10
Q

What is an orbital?

A

An orbital is a region within an atom that can hold up to two electrons with opposite spins.

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11
Q

How many electrons can fit in an orbital?

A

2

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12
Q

How many subshells are present in the s orbital?

A

1

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13
Q

How many subshells are present in the p orbital?

A

3

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14
Q

How many subshells are present in the d orbital?

A

5

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15
Q

How many subshells are present in the f orbital?

A

7

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16
Q

How many electrons are present in the s orbital?

A

2

17
Q

How many electrons are present in the p orbital?

A

6

18
Q

How many electrons are present in the d orbital?

A

10

19
Q

How many electrons are present in the f orbital?

A

14

20
Q

What is the chronological filling of orbitals in energy levels?

A 
1s
2s
2p
3s
3p
4s
3d
4p
5s
21
Q

What is Hund’s Rule?

A

Where electrons have choice between orbitals of equal energy, they will fill the orbitals singly as far as possible.

22
Q

Although the 4S orbital is filled before the 3D orbital, upon being completed the 4S level rises to a higher energy level. Therefore when electrons are being removed, they are removed from 4S (blank) 3D.

A

Before

23
Q

What is the shape of an s orbital?

A

Spherical

24
Q

What is the shape of a p orbital?

A

Dumbbell

25
Q

What group(s) in the periodic table belong to the s-block?

A

Group 1 and 2

26
Q

What group(s) in the periodic table belong to the d-block?

A

Transition metals

27
Q

What group(s) in the periodic table belong to the p-block?

A

Groups 3,4,5,6,7 and 0

28
Q

What group(s) in the periodic table belong to the f-block?

A

Lanthanum series

Actinium series

29
Q

What is meant by ‘s-block’?

A

The outer sub-shell to be filled is an s sub-shell

30
Q

What is meant by ‘p-block’?

A

The outer sub-shell to be filled is a p sub-shell

31
Q

What is meant by ‘d-block’?

A

The outer sub-shell to be filled is a d sub-shell

32
Q

First ionisation energy definition

A

The energy required to convert one mole of gaseous atoms into one mole of gaseous ions with a single positive charge.

33
Q

Second ionisation energy definition

A

The energy required to convert one mole of gaseous ions with a single positive charge into one mole of gaseous ions with a double positive charge.

34
Q

Form an equation for the first ionisation energy of an element X.

A

X(g) —–> X+(g) + e-

35
Q

Form an equation for the second ionisation energy of an ion X+.

A

X+(g) —–> X2+(g) + e-

36
Q

What factors affect the size of ionisation energy?

A
  • Nuclear charge
  • Distance of the electron from the nucleus (atomic radius)
  • Shielding effect of the inner electrons
  • Stability of filled and half-filled subshells
37
Q

What is the trend in ionisation energy across a period?

A

General trend shows an increase in ionisation energies across a period.
Due to:
• Increase in nuclear charge
• Decrease in atomic radius (as the electrons are pulled closer)
• Same number of shielding electrons (although the number of electrons increase they are only being added to the same energy level).

38
Q

What is the trend in ionisation energy down a group?

A

Ionisation energy decreases as you go down a group.
This is due to:
• Increase in atomic radius
• Better shielding from inner radius

39
Q

Third Ionisation Energy Definition

A

The energy required to convert one mole of gaseous ions with a double positive charge into one mole of gaseous with a triple positive charge.

AS Chemistry Module 1 (11 decks)

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