Structure And Bonding

Question 1

What is the charge on an electron

Answer 1

-

Question 2

What is the change on a neutron

Answer 2

0 charge

Question 3

What is the mass of: protons neutrons and electrons?

Answer 3

Protons - 1
Neutrons - 1
Electrons - 1/2000 (approx)

Question 4

How are elements ordered in the periodic table?

Answer 4

They are arranged in atomic number

Question 5

What is atomic number?

Answer 5

Number of protons

Question 6

What is atomic mass

Answer 6

Number of protons and neutrons

Question 7

Is the atomic number or atomic mass on top on the periodic table?

Answer 7

The atomic mass is on top

Question 8

Why are atoms electrically neutral?

Answer 8

Because they have the same number of positive and negative charges ( protons and electrons)

Question 9

What is the attraction of positive and negative ions?

Answer 9

The electrostatic force of attraction

Question 10

What is the charge on a proton?

Answer 10

Positive

Question 11

What is the relationship between the number of electrons in the highest energy level and the group number?

Answer 11

The number of electrons in the outer shell belong to the same group on the periodic table

Question 12

Why do atoms react and bond?

Answer 12

In order to gain a full outer shell to become stable

Question 13

How are the ions held together in eg solid magnesium oxide?

Answer 13

They are held together by the electrostatic force of attraction between positive and negative ions

Question 14

Property of diamond?

Answer 14

Hardness

Question 15

What is an element?

Answer 15

A substance which contains one type of atom

Question 16

What is the difference between a mixture and a compound?2

Answer 16

Mixtures contain more than one element

Compounds are chemically bonded mixtures aren’t

Question 17

Why are metals malleable and ductile?

Answer 17

Because metals are arranged in layers

So the layers of ions can slide over each other

Question 18

Why do metals conduct electricity?

Answer 18

Because they are held together in an see of delocalised electrons but the electrons are able to move because the electrons are free to carry charge

Question 19

Why do metals have high melting/boiling points?

Answer 19

• strong electrostatic is between positive ions and electrons that take a lot of energy to break

Question 20

What is the arrangement of metal atoms?

Answer 20

Closely packed in layers

Question 21

Physical properties of metals?6

Answer 21

• good conductor of heat and charge
• shiny
• generally hard (and solid)
• malleable
• alloys
• generally grey

Question 22

Two elements with giant covalent structures?

Answer 22

Diamond and carbon

Question 23

What state are ionic substances at at room temperature?

Answer 23

Solid

Question 24

Why do ionic substances have high boiling points?3

Answer 24

Because they form strong bonds
Because of the electrostatic force of attraction oppositely charged ions
so a lot of energy is required to break them

Question 25

Do ionic substances have low melting points?

Answer 25

No they are high

Question 26

Why will ionic compounds conduct electricity when molten or in solution?

Answer 26

Because their ions can move freely and thus carry charge through the liquid

Question 27

At room temperature what are simple molecules?

Answer 27

They are liquids or gases

Question 28

Why don't simple molecules conduct electricity? 3

Answer 28

There is overall charge on a simple molecule so they can't carry electrical charge & no free electrons

Question 29

Why do substances made up of simple molecules have low boiling points?3

Answer 29

- between molecules - there are weak intermolecular forces - not much energy is required to break them and boil the substance

Question 30

Describe an ionic lattice? 3

Answer 30

- regular arrangement ( in rows) - held together by an electrostatic force of attraction - between oppositively charged ions

Question 31

In a simple molecule what is strong and what is weak?2

Answer 31

The covalent bonds are strong | The forces between molecules are weak

Question 32

Examples of simple molecules? 4

Answer 32

CO HCl CO2 H2

Question 33

Physical properties of diamond?4

Answer 33

- very hard - very high boiling/melting point - insoluble in water

Question 34

Physical properties of graphite?3

Answer 34

Soft Slippery Conducts electricity

Question 35

Why is graphite slippery?3

Answer 35

There are weak intermolecular forces between the layers so They can then slide over eachother Making graphite soft and slippery

Question 36

Why is diamond hard?4

Answer 36

The atoms in diamond form a giant structure They form strong covalent bonds They form 4 bonds So lots of energy is required to break the bonds

Question 37

Why can graphite conduct electricity?

Answer 37

- it only makes three bonds to Carbon - this leaves a delocalised electron ( because it is arranged in layers) - can travel between the layers carrying charge

Question 38

Why can't diamond conduct electricity? 2

Answer 38

- Diamond does not have delocalised (free) electrons | - because they are all used in bonding

Question 39

How many bonds to carbon does diamond/graphite make?

Answer 39

4 and 3

Question 40

Examples of giant covalent structures?3

Answer 40

Silicon dioxide Diamond Graphite

Question 41

Describe the bonding in metals?

Answer 41

The bonding is strong because of the electrostatic force of attraction between ions and electrons

Question 42

What is a giant covalent structure?

Answer 42

A huge 3D network of covalently bonded atoms eg diamond or graphing

Question 43

What is a covalent bond?

Answer 43

A shared pair of electrons

Question 44

How is a covalent bond formed?3

Answer 44

- When an atom wants to become stable - it can covalently bond to share electrons between the atoms - to form a full outer shell

Question 45

explain the bonding in giant covalent structures?4

Answer 45

- Lots of bonds - very strong bonds - covalent bonds - held together in regular giant lattices

Question 46

Why is graphite softer than diamond?4

Answer 46

- graphite has weak intermolecular forces - graphite is in layers that can slide over eachother - in diamond each atom had no free electrons as in bonded to 4 - so no carbon atoms can slide over eachother

Question 47

What are nano particles?

Answer 47

Particles of size 1-100 nm

Question 48

Why does carbon dioxide have a low boiling point?3

Answer 48

- carbon dioxide is a simple molecule - there are weak intermolecular forces between the molecules - so not much energy is needed to break them

Question 49

How does a positively charged hydrogen ion change into a hydrogen atom?

Answer 49

Gains one electron

Question 50

Why is silicon dioxide a suitable material for lining furnaces?

Answer 50

- high melting point - lot of energy needed to break its bonds - because it has strong bonds - because it is a giant structure

Question 51

Describe the structure of a metal?

Answer 51

Sea of delocalised electrons | Positively charged metal ions

Question 52

Describe the structure and bonding of a metal?

Answer 52

Positive ions Sea of delocalised electrons That carry charge Giant lattice

Question 53

Why use a certain metal for dental braces?

Answer 53

Shape memory alloy

Question 54

How does an ion form?

Answer 54

When atoms form chemical bonds by transferring electrons

Question 55

Alkali metals react with non metals to form what?

Answer 55

Ionic compounds | In which the metal ions has a single positive charge

Question 56

What does a compound contain?

Answer 56

Two or more elements which are chemically combined

Question 57

What is a compound?

Answer 57

Substances in which 2 or more elements are chemical combined

Question 58

Why do ionic compounds have high melting and boiling points?

Answer 58

Because lots of energy is required to break the many strong bonds

Question 59

What do metals consist of?

Answer 59

Giant structure of atoms in a regular patterns | Delocalised electrons held in place by positive ions (electrostatic force of attraction)

Question 60

Describe force in ionic lattices?

Answer 60

The force exerted by an ion on other ions in the lattice acts equally in all directions

Question 61

Why are ionic structures held together so strongly?

Answer 61

Force exerted by an ion on other ions acts equally in all directions