unit 1

Question 1

relative mass of a proton

Answer 1

1

Question 2

relative mass of a neutron

Answer 2

1

Question 3

relative mass of an electron

Answer 3

1/2000

Question 4

relative charge of a proton

Answer 4

+1

Question 5

relative charge of a neutron

Answer 5

0

Question 6

relative charge of an electron

Answer 6

-1

Question 7

define mass number

Answer 7

number of protons + number of neutrons

Question 8

define atomic number

Answer 8

number of protons

Question 9

what is the principle quantum number

Answer 9

energy levels are identified by a number, the larger the number of n the further away from the nucleus and higher the energy level it is

Question 10

what do each shell contain

Answer 10

atomic orbitals

Question 11

define wave particle duality

Answer 11

electrons can behave like a wave or particle

Question 12

4 types of orbitals

Answer 12

s p d f

Question 13

features of s orbital

Answer 13

spherical. holds 2 electrons max

Question 14

features of p orbital

Answer 14

3d dumbbell shape 6 electrons max

Question 15

define subshells

Answer 15

a group of the same type of orbital with a shell
(Each new shell gains a new type of sub shell)

Question 16

max electrons s subshell can hold

Answer 16

2

Question 17

max electrons p subshell can hold

Answer 17

6

Question 18

max electrons d subshell can hold

Answer 18

10

Question 19

max electrons f subshell can hold

Answer 19

14

Question 20

max electrons in main energy level 1

Answer 20

2

Question 21

max electrons in main energy level 2

Answer 21

8

Question 22

max electrons in main energy level 3

Answer 22

18

Question 23

max electrons in main energy level 4

Answer 23

32

Question 24

what is Aufbau principle

Answer 24

Start at the lowest energy level (shell) and add electrons one at a time.

Fill each sub level before starting the next

Question 25

define isotope

Answer 25

atoms of the same element with the same number of protons but different numbers of neutrons

Question 26

Define ionic bonding

Answer 26

The electrostatic attraction between oppositely charged ions

Question 27

Define Hunds rule

Answer 27

Fill each orbital with one electron at a time before pairing electrons

Question 28

define groups

Answer 28

columns on a periodic table elements in a group have similar properties

Question 29

define electron transfer

Answer 29

occurs between metals and non metals

Question 30

in ionic bonding metals electrons and become ions, non metals electrons and become ions

Answer 30

lose, positive gain, negative

Question 31

3 properties of ionic bonding

Answer 31

strong electrostatic forces (in all directions between oppositely charged ions) high melting + boiling points when melted or dissolved in water ionic compounds can conduct electricity (ions are free to move + carry current)

Question 32

diamond features

Answer 32

all atoms in the structure are linked by strong covalent bonds high melting points each carbon forms 4 covalent bonds so very hard Doesn’t conduct electricity Tetrahedral shape

Question 33

graphite features

Answer 33

each carbon form to 3 others forming layers layers slide over each other because there no covalent bonds between layers soft and slippery 1 electron from 1 carbon is delocalised which allows conduction of heat + electricity

Question 34

define macromolecule

Answer 34

giant covalent bonds

Question 35

covalent bonding molecules properties

Answer 35

shared pair of electrons low melting and boiling point (weak intermolecular forces easier to break) doesn't conduct electricity (molecules don't have overall charge, no free electrons or ions)

Question 36

metallic bonding features

Answer 36

giant structures of atoms in a regular pattern loose electrons in outer shell (free to move) 'sea' of delocalised electrons Strong electrostatic attraction between negatively charged electrons that holds structure together

Question 37

how to work out Mr

Answer 37

add mass number of all elements present together

Question 38

%mass equation

Answer 38

mass of element/mass of compound x 100

Question 39

%yield equation

Answer 39

amount of product (actual)/max of potential (theoretical) x 100

Question 40

define empirical formula

Answer 40

simplest whole number ratio

Question 41

What is a Dative covalent bond

Answer 41

The atoms supplies both the shared pair of electrons to the covalent bond

Question 42

What is lone pair of electrons

Answer 42

Outer shell pair of electrons this is not involved in chemical bonding

Question 43

The Of a solution is a measure of how much Is dissolved of .

Answer 43

Concerntrate , solute, per unit, solvent

Question 44

Concerntration equation

Answer 44

Amount of solvent (moles)/ volume of solute (dm^3) Mass of solid / volume of liquid

Question 45

What is solute measured in

Answer 45

Moles (amount)

Question 46

Volume of solvent is measured in

Answer 46

Dm^3

Question 47

conc measured in

Answer 47

moldm^3

Question 48

1 ml to cm

Answer 48

1cm

Question 49

1000ml to litre

Answer 49

1litre

Question 50

1000ml to dm^3

Answer 50

1dm^3

Question 51

What did dimitri Mendeleev do

Answer 51

Arranged elements by atomic weight Left gaps for missing elements Elements in the same group have similar properties

Question 52

What did Henry Moseley do

Answer 52

Arranged period group in order of increasing atomic number (related to atomic mass)

Question 53

Define periodicity

Answer 53

Variation of properties of elements with changing atomic number

Question 54

What is First ionisation energy

Answer 54

The energy required to remove one electron from each atom in one mole of atoms in the gaseous state ( from 1 mole of 1+ ions) Na(g) -> Na(g) + e- Nuclear charge increases (more attraction) harder to lose electron

Question 55

What is titration

Answer 55

Neutralisation coloured water to colourless to see conc of solution