The nature of ionic bonding Flashcards Preview

AQA Chemistry (3, Bonding) > The nature of ionic bonding > Flashcards

Flashcards in The nature of ionic bonding Deck (21):
1

What are the 3 types of strong chemical bonds?

ionic, covalent and metallic

2

Why are noble gases very unreactive?

Because they have a full valence electron shell

3

How many electrons do metals have in their valence shell?

1,2, or 3

4

What is the easiest way for a metal to have a full outer shell?

To loose their valence electrons

5

What is the easiest way for a non-metal to have a full outer shell?

To gain electrons because there are gaps in their outer shell

6

What does ionic bonding occur between?

Metals and non-metals

7

How are the electrons transferred during an ionic bond?

The metal transfers their electron(s) to the non-metal

8

What type of charged ion does the non-metal become after gaining electrons from the metal?

A negatively charged ion

9

What type of charged ion does the metal become after loosing an electron to the non-metal?

A positively charged ion

10

Why and how is an attraction formed between the metal and the non-metal?

The metal looses its electrons to the non-metal, creating positively and negatively charged ions. These oppositely charged ions attract each other, creating a strong electrostatic force of attraction?

11

What kind of attraction is made between the oppositely charged ions?

A strong electrostatic force of attraction

12

What structure do ionic compounds exist as?

A lattice/giant ionic crystal

13

How is a lattice/giant ionic crystal formed?

The strong electrostatic forces of attraction between the oppositely charged ions extends throughout the compound.

14

Draw a diagram of the structure of a giant ionic crystal/lattice

A image thumb
15

What state of matter are ionic compounds at room temperature?

Solid

16

Why does a giant ionic crystal have a high boiling point?

Because there are strong electrostatic forces of attraction between the oppositely charged ions throughout the crystal which require a lot of energy to overcome/break.

17

Do ionic compounds conduct electricity?

Yes, but only when molten or dissolved in water.

18

Why is it that the ionic compound has to be molten or dissolved in water before it can conduct electricity?

It is because electricity is all about the movement of electrical charge and so the charged ions in the ionic compound must be able to move in the liquid state in order to carry this charge.

19

Why are ionic compounds brittle and shatter easily?

This because the compound is composed of alternating positive and negative ions, and, if given a sharp blow the pattern could be disrupted and positive ions and negative ions would be opposite each other. This would cause them to repel and the compound to shatter.

20

Draw a diagram to show how ionic compounds can shatter

Check pg 46

A image thumb
21

Fuse school video on the properties of ionic compounds