bonding, structure and properties of matter-paper 1

Question 1

What are Ions how are they made?

Answer 1

1)Ions are charged particles -atoms lose, gain electrons to form ions-Trying get full outer shell= stable
2)number of electrons lost or gained is the same as the charge on the ion. 2 electrons are lost=charge is 2+.

Question 2

What are cations and anions, which groups do this?

Answer 2

1)Group 1 and 2 elements are metals and they lose electrons to form positive ions (cations).
2) Group 6 and 7 elements are non-metals. They gain electrons to form negative ions (anions).

Question 3

How do you what element forms what ion?

Answer 3

.Elements same group all have the same number of outer electrons. lose or gain the same number to get a full outer shell= same

Question 4

What is Ionic Bonding ?

Answer 4

.metal and a non-metal react together
=metal atom loses electrons to form a positively charged ion
=non-metal gains these electrons=negatively charged ion.
oppositely charged ions strongly attracted by electrostatic forces=ionic bond.

Question 5

How do you draw a Dot and Cross Diagrams which Show How Ionic Compounds are Formed?

Answer 5

1)Dot and cross diagrams arrangement of electrons in an atom or ion. Each electron is represented
2)by a dot or a cross. So these diagrams can show which atom the electrons in an ion originally came from.

Question 6

1)What are ionic compunds structures?
2)How are they arranged to be held together and in what direction?
3)what is another way of showing this?

Answer 6

1)lonic compound structure=giant ionic lattice.
2)regular lattice arrangement strong electrostatic forces of attraction between oppositely charged ions-in all directions in the lattice.
3)ball and stick model showing the bonds between them

Question 7

What are Ionic Compounds Similar Properties? 4

Answer 7

1)high melting points and high boiling
=strong bonds between ions.=lots of energy to overcome this attraction.
2) solid=ions are held in place, can’t conduct electricity.
3)ionic compounds melt=ion free to move=carry electric charge.
4) Some ionic compounds dissolve in water.= ions separate all free to move solution=carry electric charge.

Question 8

Look at Charges to Find the Formula of an Ionic Compound?

Answer 8

1)dot and cross diagram, count up how many atoms there are of each element.
2) 3D diagram, use it to work out what ions are in the ionic compound

Question 9

How do Covalent Bonds work?

Answer 9

1) non-metal atoms bond together=share pairs of electrons to make covalent bonds.
2) positively charged nuclei of the bonded atoms are attracted to the shared pair electrons by electrostatic forces= very strong.
3) Each single covalent bond provides one extra shared electron for each atom.

Question 10

What are the Different Ways of Drawing Covalent Bonds?

Answer 10

Question 11

Stick model of atoms?

Answer 11

Question 12

What are simple molecular substances?

Answer 12

.made up of molecules containing a few atoms joined together covalent bonds.

Question 13

Hydrogen simple molecular substance?

Answer 13

.one electron=single covalent bonds,
.other hydrogen atoms or other elements

Question 14

Oxygen simple molecular substance?

Answer 14

.needs two electrons outer shell
=oxygen atoms share two pairs electrons double covalent bond.

Question 15

Methane simple molecular substance ?

Answer 15

.carbon= outer electrons half a full shell.
=form four covalent bonds hydrogen atoms fill up outer shell.

Question 16

Chlorine simple molecular substance?

Answer 16

.one more electron to complete the outer shell, .two chlorine atoms share one pair of electrons single covalent bond.

Question 17

Nitrogen simple molecular substance?

Answer 17

.two nitrogen atoms share three pairs of electrons creates a triple bond.

Question 18

Water simple molecular substance?

Answer 18

-oxygen shares a pair of electrons with two H atoms to form two single covalent bonds.

Question 19

Hydrogen Chloride simple molecular substance?

Answer 19

.both atoms only need one more electron to complete outer shells.

Question 20

What are the melting and boiling point Simple Molecular Substances due to covalent bonds?
How does this change as the molecules get bigger?
Do they conduct electricity?

Answer 20

1) covalent bonds usually=simple molecular structures
2) held together by very strong covalent bonds=forces of attraction between these molecules are very weak.
3) very low melt or boil=break these feeble intermolecular forces not the covalent bonds
4) molecular substances gases or liquids at room temperature.

1) molecules get bigger, strength of the intermolecular forces increases, so
more energy is needed to break them=melting and boiling points increase.

1)Molecular compounds don’t conduct electricity, simply aren’t charged=no free electrons or ions.

Question 21

What are Polymers, how to draw them?

Answer 21

.polymer=lots of small units linked together to form a long molecule=repeating sections.
2)atoms in a polymer joined by strong covalent bonds.
3)draw shortest repeating section, called the repeating unit, like this:

Question 22

What are the intermolecular forces like between polymers? 2

Answer 22

1)intermolecular forces between polymer molecules=larger than between simple covalent molecules, energy is needed to break them=most polymers are solid at room temperature.
2)intermolecular forces=weaker than ionic or covalent bonds= lower boiling points

Question 23

What are Giant Covalent Structures- macromolecules and are the 3 examples?

Answer 23

.1)Macromolecules= atoms are bonded to each other by strong covalent bonds.
2) very high melting and boiling points
3)don’t contain charged particles=don’t conduct electricity - not when molten
4) diamond and graphite (carbon atoms) and silicon dioxide (silica).

Question 24

What is Diamond?

Answer 24

.Each carbon atom forms=four covalent bonds
.rigid giant covalent structure.

Question 25

What is Graphite? 2

Answer 25

-Each carbon atom forms three covalent bonds layers of hexagons.
-Each carbon atom also one delocalised electron.

Question 26

What is Silicon dioxide?

Answer 26

.one giant structure of silicon and oxygen.

Question 27

What are Diamond properties? 3

Answer 27

= really hard.
.strong covalent bonds=very high melting point.
.doesn’t conduct electricity because no free electrons or ions.

Question 28

What are Graphite properties? 3

Answer 28

1) NO covalent bonds between the layers -weak, free to move over each other=soft, slippery,lubricating.
2) high melting point - covalent bonds layers need loads of energy to break.
3)Only three out four outer electrons are used in bonds=each carbon atom= one electron delocalised, move=conducts electricity and thermal energy.

Question 29

What is Graphene?

Answer 29

1)sheet of carbon atoms joined together in hexagons.
2)one atom thick= two-dimensional substance.
3)network of covalent bonds=very strong. incredibly light
-can be added to composite materials=improve their strength without much weight.
4)Can conduct.

Question 30

What are Fullerenes, there properties and what they can be used for? 4

Answer 30

1) Fullerenes molecules of carbon=closed tubes or hollow balls.
2) carbon atoms hexagons, pentagons or heptagons (rings of seven carbon atoms).
3) structure forms around another molecule, trapped inside=deliver a drug into the body.
4) huge surface area, make=industrial catalysts -.lubricants.

Question 31

What are nanotubes and what can they do?

Answer 31

-Fullerenes - tiny carbon cylinders.
.ratio between length diameter of nanotubes is very high
-Nanotubes can conduct, high strength
-strengthen materials without adding much weight.

Question 32

What is buckminsterfullerene what does it do{molecular formula?

Answer 32

.first fullerene to be discovered.
.molecular formula C60, forms a hollow sphere.

Question 33

What is Metallic Bonding? 2

Answer 33

1) Metals=giant structure. electrons in the outer shell of metal atoms delocalised. strong forces of electrostatic attraction between positive metal ions+shared negative electrons.
2) forces attraction hold the atoms together in a regular structure= metallic bonding=very strong.

Question 34

Why are most Metals are Solid at Room Temperature?
What does it mean to be a good conductor?

Answer 34

.1)electrostatic forces between the metal atoms and the delocalised electrons=very strong, lots of energy to be broken.
-most compounds with metallic bonds=very high melting and boiling points=solid at room temperature.
2) Good Conductors=delocalised electrons carry electric charge and thermal (heat) energy through
the whole structure,.

Question 35

Why are Metals Malleable?

Answer 35

.layers of atoms in a metal can slide over each other=metals malleable=can be bent

Question 36

Why are Alloys are Harder Than Pure Metals?

Answer 36

1)metals used everyday=alloys (mixture of two or more metals or element)=harder more useful
2) Different elements have different sized atoms. mixed with a pure metal, new metal atoms
distort the layers of metal atoms=difficult for them to slide over each other.

Question 37

What are the Three States of Matter?

Answer 37

.Solid, Liquid and Gas

Question 38

How strong the forces are depends on 3 things?

Answer 38

1)how strong forces of attraction are between particles.
2) the material structure
3)type of bonds holding particles together
4)the temperature.
5)pressure.

Question 39

Soilds properties? 3

Answer 39

1) strong forces of attraction between particles fixed position=regular lattice arrangement.
2) particles don’t move from their positions= definite shape volume
3) particles vibrate about their positions=hotter the solid becomes=more they vibrate.

Question 40

Liquids properties?

Answer 40

1) liquids=weak force of attraction. Randomly arranged+move past each other.
2) Liquids have a definite volume,don’t keep a definite shape, flow to fill the bottom of a container.
3) The particles are constantly moving with randomly: hotter the liquid=faster they move.

Question 41

Gas properties?

Answer 41

1)force of attraction between the particles is very weak - free to move, particles in gases travel straight lines.
2) Gases don’t keep a definite shape or volume always fill any container.
3)particles move constantly with random motion. hotter the gas gets, faster they move.
Gases either expand when heated, or their pressure increases.

Question 42

What is (2) wrong with the particle theory?

Answer 42

1.particles aren’t solid or inelastic and they aren’t spheres - they’re atoms, ions or molecules.
2.model doesn’t show the forces between the particles, no way of knowing how strong they are.

Question 43

What do State Symbols Tell You the State of a Substance in an Equation?

Answer 43

(s) – solid. (L) – liquid. (G) – gas. (aq) – aqueous

Question 44

What happens when a Substances Can Change from One State to Another?

Answer 44

Physical changes don’t change the particles - just their arrangement or their energy.

Question 45

What happens when a solid heats up?

Answer 45

1) .particles gain more energy particles vibrate=weakens the forces that hold solid together.
2) melting point particles have enough energy to break free=MELTING the solid turns into a liquid.

Question 46

What happens when a liquid heats up?

Answer 46

1)energy makes the particles move faster, weakens and breaks the bonds holding the liquid together.
2)boiling point, particles enough energy break their bonds/evaporating=liquid becomes a gas.

Question 47

What happens when a liquid freezes?

Answer 47

1) less energy-move less At boiling point, so many bonds formed between the gas particles gas becomes a liquid= CONDENSING
2)at melting point many bonds formed between the particles held in place. The liquid becomes a solid=FREEZING.
2)not enough energy to overcome the attraction between the particles, more bonds form between them.

Question 48

What happens when a gas cools?
What does the amount of energy needed to change state depend?

Answer 48

1) particles no longer have enough energy overcome the forces of attraction between them.
2) amount of energy needed for a substance to change state depends on how strong forces between particles are.
stronger the forces, the more energy is needed to break them=higher the melting and boiling points of the substance.

Question 49

How to Predict the State of a Substance?

Answer 49

.If the temperature’s below the melting=solid.
.above the boiling point=gas. .between the two points= liquid.

Question 50

What are Nanoparticles?

Answer 50

.Really Tiny particles contain only a few hundred atoms.

Question 51

How big is Nanoparticles SA:V is why is it important?

Answer 51

.Large Surface Area to Volume Ratio affect the way that a particle behaves.
.volume= width3 SA=Area one face (added all up)

Question 52

How to figure out SA:V ratio?

Answer 52

1)surface area to volume ratio = surface area ÷ volume
2)particles decrease in size, the size of their surface area increases in relation to their volume=surface area to volume ratio to increase

Question 53

What and how can Nanoparticles Be Used in? 5

Answer 53

1)huge surface area to volume ratio=help make catalysts.
2) Nanomedicine=tiny particles absorbed more easily by the body than most particles. deliver drugs right.
3)conduct electricity, tiny electric circuits for computer chips.
4)Silver nanoparticles have antibacterial properties=added to polymer fires used make surgical masks
5) Nanoparticles=cosmetics.

Question 54

How are Effects of Nanoparticles on Health Aren’t Fully Understood?

Answer 54

1)affect the body isn’t fully understood, important that any new products are tested minimise the risks.
2) Unsure long-term impacts on health will be.

Question 55

How are nanoparticles used in sun creams?
Two negatives?

Answer 55

1)better protecting skin from harmful UV rays.
-better skin coverage

-not clear whether nanoparticles get into your body,
-washed away damage environment.

Question 56

Ammonia structure as a molecule?

Answer 56

-hydrogen and nitrogen share one electron each x3

Question 57

Intermolecular?
Electrostatic?

Answer 57

Between molecules
Between negative and positive charges

Question 58

Writing empirical formula for ions?

Answer 58

.mg2+ need two Chlorine atoms to accept the two electrons from magnesium