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Chemistry Module 3 > Periodicity and Periodic Trends > Flashcards

Periodicity and Periodic Trends Flashcards

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1
Q

How are elements arranged in the new periodic table? (2)

A
  • Physical and chemical properties

- Atomic number

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2
Q

What is periodicity?

A

A repeating trend in properties of the elements across a period

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3
Q

What are some properties that change across a period? (4)

A
  • Electron configuration
  • Ionisation energy
  • Structure
  • Melting points
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4
Q

What is the first ionisation energy?

A

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

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5
Q

How does atomic radius affect ionisation energy?

A

As atomic radius increases, there is less attraction between the nucleus an the outer electrons. Ionisation energy decreases

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6
Q

How does nuclear charge affect ionisation energy?

A

Greater the nuclear charge, the greater attraction between the nucleus and the outer electrons. Ionisation energy increases

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7
Q

How does electron shielding affect ionisation energy?

A

More shielding means more repulsion between electrons and reduced attraction of nucleus to outermost electrons. Ionisation energy decreases

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8
Q

What is the trend as you go down a group? (4)

A
  • Atomic radius increases
  • Electron shielding increases (more electrons)
  • Nuclear attraction to outer electrons decreases
  • First ionisation energy decreases
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9
Q

What is the trend as you go down a period? (5)

A
  • Nuclear charge increases
  • Similar shielding (same shell)
  • Nuclear attraction increases
  • Atomic radius decreases
  • First ionisation energy increases
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10
Q

Why is there a drop in ionisation energy from nitrogen to oxygen? (3)

A
  • In nitrogen and oxygen the highest energy electrons are in the 2p sub-shell
  • In oxygen, the paired electrons repel each other making it easier to remove
  • In nitrogen the electrons are as far apart as possible
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11
Q

What is metallic bonding?

A

The strong electrostatic attraction between cations (positive ions) and delocalised electrons

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12
Q

What is the structure of metals? (3)

A
  • Cations in fixed places
  • Electrons are delocalised and free to move
  • Giant metallic lattice
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13
Q

Why are the properties of metals? (3)

A
  • Strong metallic bonds
  • High electrical conductivity
  • High melting and boiling points
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14
Q

Why can metals conduct electricity? (3)

A
  • Can conduct in both solid and liquid state
  • Contain delocalised electrons that can move through the structure
  • Electrons carry the charge across the metal
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15
Q

Why do metals have high melting and boiling points? (2)

A
  • High temperatures necessary to provide large amount of energy needed to overcome the strong electrostatic attraction between cations and anions
  • Strong attraction means more energy needed
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16
Q

Are metals soluble?

A

No, they just react with solvents

17
Q

What is a giant covalent lattice?

A

Many atoms being held together by a network of strong covalent bonds

18
Q

What are the properties of giant covalent lattices? (

A
  • High MP/BP - Strong covalent bonds require high temps. to provide enough energy to break
  • Insoluble - covalent bonds are too strong to be broken by interactions with solvents
  • Do not conduct electricity (EXCEPT Graphite and Graphene) - no available electrons to carry the charge across the molecule
19
Q

What is the structure of graphite? (2)

A
  • Hexagonally arranged carbon atoms

- Parallel layers held together by weak London forces

20
Q

What is the structure of graphene? (2)

A
  • Single layer of graphite

- Hexagonally arranged carbon atoms

21
Q

Why can graphite and graphene conduct electricity? (3)

A
  • The bonding only uses three out of four electrons on the carbon
  • One free electron left
  • Free electron is free to move across the molecule and carry the charge
22
Q

Why is there a sharp decrease in the periodic trend in melting points?

A

Point marks a change between giant to simple molecular structures

23
Q

What elements form giant metallic structures? (5)

A
  • Li
  • Be
  • Na
  • Mg
  • Al
24
Q

What elements form giant covalent structures? (3)

A
  • B
  • C
  • Si
25
Q

What elements form simple molecules? (8)

A
  • N2
  • O2
  • F2
  • Ne
  • P4
  • S8
  • Cl2
  • Ar

Chemistry Module 3 (1 decks)

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