Bonding Structure And Properties Of Matter R

Question 1

What are the three types of strong chemical bonds

Answer 1

Ionic bonds

Covalent bonds

Metallic bonds

Question 2

What are atoms that have gained or lost electrons called

Answer 2

Ions

Question 3

What do Ionic bonds occur between

Answer 3

Positive and negative ions

Question 4

What type of outer shell do ions have and why?

Answer 4

Full,due to ions always having a charge due to losing or gaining electrons giving it the charge

Question 5

Ionic binding involves a transfer of electrons from ____atoms to ______atoms

Answer 5

Metals

Non-metals

Question 6

What type of force of attraction is an ionic bond

Answer 6

Electrostatic force of attraction

Question 7

What are ionic compounds giant structures of

Answer 7

Ions

Question 8

What are ionic compounds held together by

Answer 8

Strong ionic compounds

Question 9

What are feature of ionic compounds

Answer 9

Have high melting and boiling points

Don’t conduct electricity when solid due to ions can’t move

Conduct electricity when dissolved or molten because charged ions are free to move about and carry their charge

Question 10

Where does metallic binding occur

Answer 10

Metallic elements such as iron and copper

Alloys, such as stainless steel

Question 11

What does delocalised electron mean?

Answer 11

Not bound to one atom

Question 12

Why can metals conduct electricity surprisingly well for a solid

Answer 12

Die to many delocalised electrons which travel between each molecule to transfer the electricity

Question 13

what is a lattice of positive ions held together by

Answer 13

electrostatic attraction

Question 14

what type of bond is pulling together the positive ions and delocalised electrons

Answer 14

metallic bond

Question 15

why are metals useful as structural materials

Answer 15

metallic bonds are very strong and metals have high melting and boiling points

Question 16

what type of particle arrangements are in pure metals

Answer 16

a regular arrangement

Question 17

why are pure metals easily bent

Answer 17

the layers slide over eachother quite easily

Question 18

why is copper traditionally made to make water pipes

Answer 18

• it is an unreactive metal,so does not react with water

- it can be easily shaped

Question 19

what are the uses for aluminum

Answer 19

high-voltage power,cables,furniture,drinks cans,foil food wrap

Question 20

what are the properties of aluminium

Answer 20

corrosion resistant,ductile,malleable,good conductivity,low density

Question 21

what are the uses for copper

Answer 21

electrical wiring,water pipes,sauce pans

Question 22

what are the properties of copper

Answer 22

ductile,malleable,good conductivity

Question 23

what are the uses for gold

Answer 23

jewellery,electrical junctions

Question 24

what are the properties of gold

Answer 24

ductile,shiny,god conductivity

Question 25

what are most metal objects made from?

Answer 25

alloys

Question 26

what do alloys do?

Answer 26

the added element to the pure metal disturbs the weak regular arrangement of the metal atoms so the metal atoms dont slide over eachother so recently

Question 27

What are transition metals

Answer 27

Metals which have a partially filled outer shell

Question 28

Where can transition metals be found

Answer 28

The middle of the periodic table

Question 29

What is a covalent bond

Answer 29

A shared pair of electrons between atoms

Question 30

Where do covalent bonds occur in

Answer 30

Non metallic elements and compounds of non metals

Question 31

If a chlorine atom has seven electrons in its outer shell in order to bind with another chlorine atom what must happen

Answer 31

An electron from each atom is shared This gives chlorine atom eight electrons in the outer shell Each atom now has a complete outer shell

Question 32

How can covalent bonds in molecules be shown

Answer 32

Dot and cross diagrams

Question 33

Are covalent bonds weak or strong

Answer 33

Strong

Question 34

What do simple molecules contain

Answer 34

A relatively small no. Of non metal atoms joined together by covalent bonds

Question 35

What usually are substances that consist of simple molecules

Answer 35

Liquids and gases that have relatively low melting and boiling points

Question 36

Why do simple molecules have low melting and boiling points

Answer 36

They have weak intermolecular forces

Question 37

If a molecule is large is the intermolecular forces stronger or weaker

Answer 37

Stronger

Question 38

What happens when you go down group 7 of the periodic table

Answer 38

The molecules get larger and melting points increase due to stronger intermolecular forces

Question 39

At room temp. What is fluorine

Answer 39

Gas

Question 40

At room temp.what is bromine

Answer 40

Liquid

Question 41

At room temp. What is iodine

Answer 41

Solid

Question 42

What are atoms in giant covalent structures linked by

Answer 42

Strong covalent bonds

Question 43

What is a giant covalent structure

Answer 43

A giant covalent structure is a three-dimensional structure of atoms that are joined by covalent bonds

Question 44

What must happen to the bonds in giant covalent structures for it to melt or boil

Answer 44

They must be broken

Question 45

What do all the strong covalent bonds mean in a diamond

Answer 45

All the strong covalent bonds mean that it is a very hard substance with a very high melting point

Question 46

What type of structure should diamond have

Answer 46

It has a giant,rigid covalent structure

Question 47

What does each carbon atom form in diamond

Answer 47

Each carbon atom forms four strong covalent bonds with other carbon atoms

Question 48

What is diamond unable to do without charge particles

Answer 48

There are no charged particles so it does not conduct electricity

Question 49

In graphite what does each carbon atom form

Answer 49

Three covalent bonds with other carbon atoms

Question 50

What type of shape does graphite have

Answer 50

A layered hexagonal structure

Question 51

What is layers in graphite held together by

Answer 51

Weak intermolecular forces

Question 52

What doe is mean if graphite has weak intermolecular forces between kayers

Answer 52

The layers can slide past eachother ,making graphite soft and slippery

Question 53

One electron from each carbon atom in graphite is ____________

Answer 53

Delocalised

Question 54

What do delocalised electrons allow graphite to conduct

Answer 54

Heat and electricity

Question 55

What type of structure does silicon dioxide have

Answer 55

A lattice structure similar to diamond

Question 56

In silicon dioxide what is each oxygen atom joined to

Answer 56

Two silicon atoms

Question 57

In silicon dioxide what is each silicon atom joined to

Answer 57

Four oxygen atoms