Bonding, Structure and Properties of Matter

Question 1

what are ions

Answer 1

ions are charged particles

Question 2

how do metals form ions and what ions do they make

Answer 2

they lose electrons from their outer shell to form positive ions

Question 3

how do non metals form ions and what ions do they make

Answer 3

they gain electrons into their outer shell to form negative ions

Question 4

what is ionic bonding and what happens

Answer 4

ionic bonding is the transfer of electrons from a metal and a non metal. The metal atom loses an electron to form a positively charged ion and the non metal gains these electrons to form a negatively charged ion.

Question 5

how can you show how ionic compounds are formed

Answer 5

dot and cross diagrams

Question 6

what structure do ionic compounds have

Answer 6

giant ionic lattice

Question 7

what’s inside an ionic compound

Answer 7

the ions inside an ionic structure form a closely packed regular lattice arrangement and there are strong electrostatic forces of attraction between oppositely charged ions in all directions in the lattice

Question 8

properties of ionic compounds

Answer 8

high melting and boiling point because of the strong bonds between them
can only conduct electricity when molten or dissolved because the ions need to be free to move

Question 9

what is covalent bonding

Answer 9

covalent bonding is the sharing of electrons between two non metals so that they can have a full outer shell

Question 10

properties of simple molecular substances

Answer 10

very strong covalent bonds but have weak intermolecular forces
low melting and boiling points because of the weak intermolecular forces
do not conduct electricity

Question 11

what is a polymer

Answer 11

are many monomers joined together

Question 12

how are atoms in a polymer joined together

Answer 12

by strong covalent bonds

Question 13

giant covalent structures properties (3)

Answer 13

strong covalent bonds
very high melting and boiling point
do not conduct electricity

Question 14

what are allotropes

Answer 14

allotropes are different structural forms of the same element in the same physical state

Question 15

diamond properties 4 things

Answer 15

made up of carbon atoms
each carbon atom forms four covalent bonds making them very hard
very high melting point because of the strong covalent bonds
does not conduct electricity as it has no free electrons

Question 16

graphite properties (6)

Answer 16

made up of carbon atoms
each carbon make 3 covalent bonds
graphite is in sheets
theyre soft due to the layers being able to slide over each other
conducts electricity due to the spare electron
high melting point

Question 17

graphene 3 things

Answer 17

is a single sheet of carbon atoms
very strong because of its network of covalent bonds but very light which makes it useful
contains delocalised electrons which makes it able to conduct electricity

Question 18

what are fullerenes

Answer 18

fullerenes are molecules of carbon

Question 19

uses of fullerenes 3 things

Answer 19

can be used to cage other molecules this can be used to deliver drugs
can be used as a catalysts because of its huge surface area
good lubricants

Question 20

metallic bonding

Answer 20

metals are made up of positive atoms in a sea of delocalised electrons

Question 21

properties of compounds with metallic bonds (4)

Answer 21

strong electrostatic forces
high melting and boiling point
good conductors of heat and electricity
the metals are malleable

Question 22

why are alloys more useful than pure metals

Answer 22

alloys are much harder than pure metals as they are a mixture between two or more metals or a metal and another element
pure metals are too soft

Question 23

why are alloys harder that pure metals

Answer 23

when another metal is mixed with a pure metal to make an alloy the new metal atoms will distort the layers of metal atoms making it more difficult for them to slide over each other. This makes alloys harder than pure metals.

Question 24

Why is iron described as an element?

Answer 24

because iron is made up of only one type of atom

Question 25

The three metals in stainless steel have different sized atoms. Stainless steel is harder than pure iron.

Answer 25

the structure of stainless steel is distorted making it hard for the layers to slide over each other

Question 26

Name the instrument used to identify the compounds.

Answer 26

mass spectrometer

Question 27

Give one reason why instrumental methods of analysis are used to identify the compounds

Answer 27

more accurate

Question 28

Suggest two conditions which could be changed when poly(ethene) is made.

Answer 28

pressure | temperature`

Question 29

2 KI(aq) + Pb(NO3)2(aq) → 2 KNO3(aq) + PbI2(s) why is this reaction a precipitation

Answer 29

a solid was formed

Question 30

How can the precipitate be removed from the reaction mixture?

Answer 30

filtering

Question 31

Describe the structure of a metal. | 3

Answer 31

lattice of positive ions with delocalised electrons

Question 32

alloy =

Answer 32

mixture of metals

Question 33

Bronze is an alloy of

Answer 33

copper and tin

Question 34

What is the carat number of pure gold?

Answer 34

24

Question 35

A nanodiamond contains a few

Answer 35

hundred atoms

Question 36

in diamond ______ atoms are bonded together

Answer 36

all

Question 37

Explain why chlorine (Cl2) is a gas at room temperature, but sodium chloride (NaCl) is a solid at room temperature.

Answer 37

chlorine covalent bonds between the atoms forming simple molecules. there is a weak attraction between the molecules meaning that it has a low boiling point sodium chloride electrostatic attraction in all directions between oppositely charged ions forming a giant lattice. large amount of energy needed to break the bonds, it has a high boiling point

Question 38

Pb(NO3)2(aq +K2CrO4(aq)⟶PbCrO4(s)+2KNO3(aq) | what would you see

Answer 38

a precipitate

Question 39

Na2CO3(aq) + 2HCI(aq)⟶2NaCl(aq) +CO2(g)+H2O(I) | Explain why this student’s results would not appear to support the law of conservation of mass.

Answer 39

co2 is a gas the gas escapes during the reaction so the mass at the end is less than expected

Question 40

In silicon dioxide, each silicon atom is bonded with ____ oxygen atoms.

Answer 40

four

Question 41

describe the structure and bonding of a metal.

Answer 41

giant structure made up of positive ions surrounded by delocalised electrons with strong bonds so a lot of energy is needed to break these bonds

Question 42

Like graphite, each carbon atom in the carbon nanotube is joined to three other carbon atoms. Explain why the carbon nanotube can conduct electricity.

Answer 42

it has delocalised electrons | it has one non bonded electron from each atom

Question 43

explain why graphite conducts electricity

Answer 43

graphite is made out of carbon atoms each carbon atom forms 3 covalent bonds one electron per carbon is delocalised these electrons carry charge through the graphite

Question 44

explain why you would not expect titanium chloride to be a liquid at room temperature

Answer 44

titanium is a metal chloride metal chlorides are usually ionic so metal chlorides are solid at room temperature because they have strong forces between ions