C2.2

Question 1

How can you differentiate between metal and non metal oxides?

Answer 1

Metal oxides are alkaline, non metal pxides are acidic

Question 2

What side of the periodic table is non-gases

Answer 2

Right side,although hydrogen is on the left

Question 3

What are properties of metal?

Answer 3

Shiny
High melting/boiling point
Solid at room temp
Malleable
Ductile
Conductors

Question 4

What does a period tell you about an element?

Answer 4

The period is the number of electron shells

Question 5

What does a group tell you about an element?

Answer 5

The group is the number of electrons in the outer shell (non IUPAC)

Question 6

What is the electron structure of an element with 15 electrons?

Answer 6

2.8.5

Question 7

If an element loses electrons,what charge does it become?

Answer 7

Positive

Question 8

If an element gains electrons,what charge does it become?

Answer 8

Negative

Question 9

How do you draw dot and cross diagrams for ionic compounds

Answer 9

Draw the outer shell of each atom
With one element being crosses and the other dots
One shell should be empty and the other full
Brackets outside the atom and shells with a + or - charge and magnitude (e.g +2)

Question 10

What are the limits of electrons in each shell?

Answer 10

Shell 1 - 2
Shell 2 - 8
Shell 3 - 8
Shell 4 - 16

Question 11

If an element X with 15 electrons reacts with an element Y with 13 electrons,what happens?

Answer 11

Y gives 3 electrons to X
They both stabilise and become positive or negatively charged
Forces of attraction bring them together

Question 12

What is the structure of ionic compounds?

Answer 12

Giant ionic lattice, positive and negative ions in a regular arrangement and alternating

Question 13

What is a simple molecule

Answer 13

A molecule with only a few atoms

Question 14

What is a covalent bond?

Answer 14

When 2 non-metals share electrons to become stable

Question 15

Give an example of a double covalent bond

Answer 15

Carbon dioxide (CO2)

Question 16

Why is the melting point of simple bolecules low even though they have covalent bonds?

Answer 16

Even though they have strong covalent bonds the intermolecular forces between the molecules are weak

Question 17

What is a giant covalent structure?

Answer 17

Many non metal atoms joined by covalent bonds,arranged in a repeating regular pattern called a giant lattice

Question 18

Why does diamond have a high melting point?

Answer 18

The atoms are covalently bonded and require a lot of energy to break apart

Question 19

Why is the empirical formula of Diamond and Graphite just C?

Answer 19

The only atoms are carbon (C), so instead of writing a high number it can just be simplified to C

Question 20

What are polymers?

Answer 20

Monomers joined together by covalent bonds, end to end in a long chain

Question 21

How do you convert a monomer displayed formula to a polymer displayed formula?

Answer 21

Remove a covalent bond from the middle,and add one reaching out on both edges
Put the formula in a bracket with n written in subscript

Question 22

What is the difference between thermosoftening and thermosetting polymers

Answer 22

In thermosoftening, polymers are simply tangled together with no extra bonds, so they have e,g a low melting point.
In thermosetting,polymers are joined by strong crosslinks (covalent bonds) , so they have e.g a high melting point

Question 23

What is the structure of metals like?

Answer 23

Atoms packed together in a giant metallic lattice

Question 24

What are metallic bonds?

Answer 24

Metal atoms lose electrons from their outer shell, which become delocalised.
There are forces of attraction between positive metal ions and delocalised electrons

Question 25

Why can metal ions conduct electricity?

Answer 25

Due to delocalised electrons which can carry charge

Question 26

How did Mendeleev initially arrange the periodic table?

Answer 26

He arranged in increasing atomic weight, but switched some elements around to fit their properties
And he grouped elements with similar properties

Question 27

How is the modern periodic table arranged?

Answer 27

In order of increasing atomic number (protons)

Question 28

Why are some elements more reactive than others?

Answer 28

It depends on how many electrons they need to gain/ lose to become stable,if it is more then they will be more desperate for reaction

Question 29

What are halogens?

Answer 29

The elements in group 7

Question 30

Why would an element with 20 electrons and an element with 12 electrons have different reactivity but still the same number of electrons in the outer shell?

Answer 30

The element with 20 electrons would be more reactive as the outer shell is further from the nucleus so it would lose those electrons easier