Chemistry Unit 2 Flashcards Preview

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Flashcards in Chemistry Unit 2 Deck (18):
1

(C2.1.1) In metallic bonding, _______ electrons from the outer shell of metal atoms form a sea of free electrons surrounding positively charged metal ions. Fill in he missing word.

Delocalised

2

(C2.1.1) How would the ions be arranged in the ionic compound sodium chloride?

Giant, regular lattice

3

(C2.1.1) A molecule contains millions of charged particles which are held together by strong forces of attraction which acts in all direction. What sort of binding is this?

Ionic bonding

4

(C2.1.1) More complicated ionic compounds can be formed from three or more elements. What is the overall charge of Calcium Carbonate (CaCO3)?

0

5

(C2.2.1) What do molten ionic compounds, dissolved ionic compounds, metals and graphite all have in common which allows them to conduct electricity?

Charged particles

6

(C2.2.1) A substance is a liquid at room temperature and does not conduct electricity.
What structure does the substance likely have?

Simple covalent structure

7

(C2.2.2) What is the boiling point range of a typical ionic compound?

1000 - 2000 degrees Celsius

8

(C2.2.2) Why can sodium chloride (NaCl) conduct electricity when it is dissolved in water?

Na and Cl ions can move around the water.

9

(C2.2.2) Why does supplying energy to a solid ionic compound allow it to conduct electricity?

Overcomes attractive forces between ions.

10

(C2.2.2) How is the structure of an ionic compound?

Regular Lattice

11

(C2.2.3) What property of graphite allows it to act as a lubricant?

There are no covalent bonds between carbon layers.

12

(C2.2.3) Name three properties of diamond that makes it well suited for use in jewellery?

Hard, Shiny and Transparent.

13

(C2.2.3) Which forces in graphite gives it it's 'slippery' properties?

Weak intermolecular forces between layers

14

(C2.2.3) A giant covalent substance is made from silicon and oxygen atoms and is used to make construction materials. What is this substance?

Silica

15

(C2.2.4) Remember:

The atoms are more ordered in a pure metal than in an alloy.

16

(C2.2.4) Why is pure iron so soft?

Regular layers of iron ions slide over each other easily

17

(C2.2.4) What quickly travels through a metallic lattice to conduct electricity and heat?

Electrons

18

(C.2.2.4) What property of the layers of metal ions in metallic structures allow metals to be easily shaped?

They distort