Periodic Trends and Bonding Flashcards Preview

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Flashcards in Periodic Trends and Bonding Deck (21)
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1
Q

Valency/valence number

A

Number electron an atom needs to lose, gain/share to achieve octet structure

2
Q

Valence electrons

A

Electrons in the outermost energy level

3
Q

Atomic radius

A

The distance between the centre of the nucleus to the outermost shell

4
Q

Ionisation energy

A

Amount of energy required to remove an electron (from a neutral atom in a gaseous state)

5
Q

Electron affinity

A

Amount of energy required to add an electron (to a neutral atom in a gaseous state)

6
Q

Electronegativity

A

How strongly atoms attract electrons

7
Q

Periodicity

A

The gradual change in physical and chemical properties of elements

8
Q

Electron Affinity:

Increases from ___ to ___ and from ___ to ___

A

Increases from left –> right and from bottom –> top

F has the highest electron affinity (top right).

9
Q

Electronegativity:

Increases from ___ to ___ and from ___ to ___

A

Increases from left –> right and from bottom –> top

F is the most electronegative (top right).

10
Q

Ionisation energy:

Increases from ___ to ___ and from ___ to ___

A

Increases from left –> right and from bottom –> top

F has the highest ionisation energy (top right).

11
Q

Atomic radius:

Increases from ___ to ___ and from ___ to ___

A

Increases from right –> left and from top –> bottom

Fr has the largest atomic radius (bottom left).

12
Q

Reactivity

A

How violently an atom reacts with another substance’s atoms

13
Q

Ion

A

An element with a charge

14
Q

Isoelectric

A

Atoms with the same electron configuration = same amount of electrons

15
Q

Rank these in decreasing ion size:

Neutral, Anion, Cation

A

Anion
Neutral
Cation

16
Q

What are the exceptions for Ionisation energy?

A
  • Elements that are equally distant cannot be identified which one has a higher IE.
  • Group 2A has higher IE than Group 3A. Group 5A has a higher IE than Group 6A.
17
Q

What is tiebreaker in electronegativity is both elements are equally distanced from fluorine?

A

The one that is higher up is more electronegative.

18
Q

What are the exceptions for Electron Affinity?

A
  • Group 1A has a higher electron affinity Group 2A.

- Group 4A has a higher electron affinity Group 5A.

19
Q

Properties of Covalent compounds

A
  • Lower melting and boiling points than ionic bonds
  • More flexible than ionic compounds
  • Not soluble in water
  • Doesn’t conduct electricity
20
Q

Properties of Ionic compounds

A
  • Arranged in crystal lattice structure
  • Solids are crystalline at room temperature
  • High melting and boiling points
  • Brittle
21
Q

Properties of Metallic compounds

A
  • Shiny
  • Conduct electricity
  • Conduct heat
  • High density
  • Malleable and ductile
  • High melting point