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Flashcards in Atomic Structure and Bonding Deck (63)
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1

What does the shell contain

Electrons

2

How can compounds form?

Energy transfer

3

How can you break an ionic compound?

Provide enough energy

4

Why is there a stronger force of attraction between MgO than NaCl?

It is mg2+O2- so there is a stronger force of attraction between the oppositely charged ions. Because there are larger opposite charges

5

What is electrical current?

The movement of charged particles such as ions or electrons in a circuit.

6

How many bonds can an atom form?

As many bonds as there are electrons in its outermost shell.

7

What is a covalent bond?

A shared pair(s) of electrons between 2 atoms. There is an attractive force between the pair of electrons and the protons in the nuclei of the atoms involved in forming the bonds.

8

What does the nucleus contain?

Protons and neutrons

9

What is an intermolecular force?

The forces of attraction between separate molecules. They can be repulsive.

10

What is an atom?

The defining structure of an element made up of protons, neutrons and electrons. The smallest part of a chemical element that can exist.

11

What is a molecule?

A fixed number of covalently bonded atoms.
(Two or more covalently bonded atoms)

12

What is metallic bonding?

The electrostatic force of attraction between positive metal ions and the sea of delocalised electrons

13

Why are metals good conductors of electricity?

Because they have a sea of delocalised electrons that are free to move where current can pass through

14

Give 3 examples of a giant covalent structure

Carbon (diamond)
Carbon (graphite)
SiO2

15

In a simple molecule what do you have to break to melt the substance?

Intermolecular forces of attraction

16

Why are metals malleable?

The layers of ions can slide over each other easily.

17

How many other carbon atoms is each carbon atom bonded to in diamond?

4

18

How many carbon atoms is each carbon atom bonded to in graphite and what does this mean?

3, that there is a delocalised electron

19

What are the forces of attraction between layers of graphite like?

Weak

20

Why is graphite a good conductor of electricity?

Because of the delocalised electrons that haven't been used and the current can pass through

21

What is graphene?

One layer of graphite

22

Why do giant covalent structures have such a high melting point

Because to melt it you need to break every covalent bond in the giant structure

23

What is the force of attraction between the metallic ions and delocalised electrons?

Electrostatic force of attraction

24

Give an example of a giant ionic structure

Sodium chloride
Anything else

25

Describe the diagram of a metallic bond

Layers of positively charged ions surrounded by a 'sea' of delocalised electrons
Layers of ions in a giant structure
i.e. circles with plus signs in with a label around saying sea of delocalised electrons

26

Give an example of a simple molecular structure

H2O

27

Why do ionic substances have a high melting point?

Because it is a giant ionic structure so more energy is required to break the attractive forces (electrostatic forces of attraction) between the positively and negatively charged ions.

28

Why do metals have a high melting point?

Because more energy is needed to break the strong electrostatic forces of attractions (bonds) between the metal ions and sea of delocalised electrons.

29

Why do simple molecular substances have low melting points?

Because only enough energy is needed to break the weak intermolecular forces between molecules

30

Do all covalent bonds conduct electricity?

NO (except graphite and graphene)