C1

Question 1

For each electron shell 1-5 what is the maximum number of electrons

Answer 1

1-2
2-8
3-18
4-32
5-50

Question 2

What is an orbital

Answer 2

Regions where there Is 95 percent probability of locating an electron
An orbital can hold up to two electrons
There are s,p,d,f orbitals

Question 3

What is electron figuration

Answer 3

The distribution of electrons in an atom/molecule

Question 4

Ionic bonding

Answer 4

Electrostatic attraction between two oppositely charged ions

Question 5

What group are nobles gases

Answer 5

0

Question 6

What is the main feature about noble gases and how does this make it different to other elements in other groups

Answer 6

Have full outer shells which means they do not react easily and do not react at all compared to other elements that do not have outer shells which allows them to react to gain stable electronic configurations

Question 7

What is a giant ionic lattice

Answer 7

Regular arrangement of positive and negative ions

Question 8

When does the electrostatic force become stronger in a ionic bond

Answer 8

When the ionic charge is higher

Question 9

When does the electrostatic force become weaker in an ionic bond

Answer 9

When the ionic radii are bigger as when the ionic radius is bigger the ionic charge is spread over a large surface area

Question 10

What is covalent bonding

Answer 10

Occurs between two non metals it forms when an electron is shared between atoms

Question 11

What is a dative covalent bond

Answer 11

When covalent molecules sharing electrons that come from one atom. For example oxygen and oxygen

Question 12

What is a triple covalent bond

Answer 12

When three pairs of electrons are shared

Question 13

What bond is stronger out of single,double or triple covalent bond and why

Answer 13

Single bonds have a greater length than double and double has a greater length than triple. The shorter the length of the bond the stronger it is

Question 14

What is a lone pair

Answer 14

A non binding electron/ electrons that haven’t been joined to a different shell

Question 15

Organic compound

Answer 15

Compound that contains one or more carbons

Question 16

What structure does methane have and why

Answer 16

Tetrahederal structure as the bonds are separated because the negative electrons repel from one another
It is a 3d shape

Question 17

Metal held by

Answer 17

Structures of atoms are held by metallic bonding

Question 18

Delocalised electron

Answer 18

Electrons that are free to move and are present in metal but no covalent bonds or single atoms

Question 19

What does delocalised electrons allow in metallic bonding

Answer 19

Gives the metal nuclei a positive charge which is attracted to the negative charge on the delocalised electrons which creates a strong force of attraction

Question 20

Is metallic bonding stronger than covalent or ionic

Answer 20

No

Question 21

How can you determine what type of bond will form between two atoms

Answer 21

Electrongetavity as it has the tendency to attract a bonding pair of electrons

Question 22

If atoms have similar electronegativities what do they form

Answer 22

Covalent bond

Question 23

Non-polar meaning

Answer 23

A molecule where the electrons are distributed evenly throughout the molecule which means in a covalent bond when the electrons have been shared between them to make the atom stable and must have the same electronegativity

Question 24

Polar covalent meaning

Answer 24

Uneven electron distribution as shared electrons are more attracted to one nucleus more than the other. The atom with higher electronegativity will attract more electrons which gives the atom a slight negative charge and the other will have a slight positive charge

Question 25

Intermolecular force

Answer 25

Th attraction/repulsion between neighbouring forces

Question 26

One type of intermolecular force

Answer 26

London dispersion forces/temporary dipole-induced dipole forces

Question 27

What is a London dispersion force

Answer 27

Weak forces between non-polar covalent molecules

Question 28

What is a dipole

Answer 28

Separation of charges within a covalent molecule

Question 29

What causes a temporary diple

Answer 29

When the electrons distribution becomes non-symmetrical

Question 30

Due to the electrons having a temporary dipole what can happen to the electrons in a nearby molecule

Answer 30

Repels the electrons which induces(causes) a dipole in that molecule

Question 31

Once there is an induced dipole what happens between it and the temporary dipole

Answer 31

Attract each other and pull the molecules together but forces are temporary as the electrons are constantly moving so electron density in the molecule is changing Larger molecules have more electrons which means the force is bigger

Question 32

When is there london dispersion forces

Answer 32

Forces that exist between noble gases and non polar molecules

Question 33

What r the main 4 points of london dispersion forces

Answer 33

If there are more electrons there is more movement which leads to bigger dipoles and a stronger attraction

Question 34

What are dipole-dipole forces and are they stronger than London dispersion forces

Answer 34

Permanent forces between polar molecules Yes they are stronger but weaker than covalent bonds

Question 35

What molecules does there have to be to be a dipole-dipole force

Answer 35

Hydrogen chloride and iodine monichloride Plus the chlorine atom is slightly negative and the hydrogen and iodine atoms are slightly positive

Question 36

What is the strongest intermolecular force

Answer 36

Hydrogen bond

Question 37

When will hydrogen bonds form

Answer 37

When compounds have hydrogen bonded to fluorine, oxygen or nitrogen as there is a large difference in electronegativity between hydrogen and these atoms

Question 38

What does this large difference lead to

Answer 38

Polar bonds are formed and so the molecules have permanent dipoles and there will be an attraction between the positive side and lone pair side

Question 39

Calculation for mass

Answer 39

Mass=molar mass×number of moles

Question 40

Relative atomic mass

Answer 40

Tells you how much mass there is in one mole of the element

Question 41

Relative formula mass

Answer 41

Sum of all the relative atomic masses of all atoms in formula

Question 42

Standard solutions

Answer 42

Using solution of a known concentration as these have been prepared to ensure specific concentration is needed

Question 43

Concentration formula

Answer 43

Number of moles of solute divided by volume of solvent

Question 44

Titration

Answer 44

A method used to calculate concentration of a solution

Question 45

Solution

Answer 45

A liquid mixture where a solute is dissolved in a solvent

Question 46

Solute

Answer 46

Substance dissolved in a solvent to form a solution

Question 47

Solvent

Answer 47

A liquid that dissolveelsbanother substance

Question 48

What does s,l,g mean next to an equation

Answer 48

Solid,liquid and gas

Question 49

What does aq mean next to an equation

Answer 49

Solution

Question 50

Stochiometry

Answer 50

Using relationships between reactants and products in a chemical reaction to work out how much product will be produces from given amounts of reactants

Question 51

Theoretical mass

Answer 51

The expected amount of product from a reaction calculated from balanced equation

Question 52

Why do people use the percentage yield equation

Answer 52

To know how efficient their reaction process is

Question 53

Percentage yield equation

Answer 53

Actual mass /theoretical mass ×100

Question 54

Ionisation energy

Answer 54

Energy requited to remove one mole of electrons from atoms in their gaseous state

Question 55

How does an atom turn into an ion

Answer 55

Gains electrons

Question 56

What is a transition metal

Answer 56

Metals rhat form more than one stable ion with an incomplete d sub shell They a re a subset of d block elements D block elements are elements where the last two electrons to fill the atom is placed into a d orbital Incomplete d sub shell explains some fo the key properties or transition metals

Question 57

How does gold conduct electricity

Answer 57

Metallic structure Delocalised electrons Electronsnare free go move Electrons carry current

Question 58

Whay foes it mean if the proton does not have a whole number

Answer 58

Different isotopes Isotopes have different abduncies Relative mass is weighed averagely

Question 59

Redox reaction

Answer 59

Oxidation and reduction Explain what what are

Question 60

How do delocalised electrons affect thermal or conduct of electrocity

Answer 60

Electricity the delocalised electrons Carey the charge good example is copper Delocalised electrons are good to absorb heat energy which gives them kinetic energy which is transferred through the metals by these electrons