2.1, 2.2, 2.3

Question 1

Name the three subatomic particles

Answer 1

1) Protons
2) Neutrons
3) Electrons

Question 2

What is the charge for protons

Answer 2

• Positively charged (1+)

Question 3

What is the charge for neutrons

Answer 3

• They have no charge (0)

Question 4

What is the charge for electrons

Answer 4

• Negatively charged (1-)

Question 5

Why do we use relative masses to measure the masses of the sub atomic particles

Answer 5

• because the sub atomic particles are too small to be measured empirically

Question 6

What is the relative mass of protons and neutrons

Answer 6

1

Question 7

What is the relative mass of electrons

Answer 7

• they have a negligible mass of 1/1836

Question 8

Where are protons located

Answer 8

• in the nucleus

Question 9

Where is the neutron located

Answer 9

• in the nucleus

Question 10

Where is the electron located

Answer 10

• in the orbital

Question 11

Define the atomic number

Answer 11

• the number of protons in the nucleus

Question 12

Define the atomic mass number

Answer 12

• the total number of protons and neutrons in the atom

Question 13

How do you work out the amount of neutrons

Answer 13

Atomic mass number — Atomic number

Question 14

Which number is always the atomic mass

Answer 14

• the bigger number ( includes total number of protons and neutrons)

Question 15

Define isotopes

Answer 15

• atoms of the same element with the same proton number but different numbers of neutrons and therefore different masses

Question 16

What do all isotopes have the same and what does this mean

Answer 16

• same ELECTRONIC CONFIGURATION and so the same chemical properties

Question 17

What do isotopes have that are different and why

Answer 17

• different physical properties because they have different masses

Question 18

Define relative isotopic mass

Answer 18

• the WEIGHTED MEAN MASS of one ISOTOPE compared to 1/12th of the mass of one atom of carbon-12

Question 19

Define relative atomic mass

Answer 19

• the WEIGHTED MEAN MASS of an atom compared to 1/12th of the mass of one atom of carbon-12

Question 20

What two things does relative atomic mass take into account

Answer 20

1) % abundance of each isotope
2) relative isotopic mass of each isotope

Question 21

Define relative molecular mass

Answer 21

• the AVERGAE MASS of a MOLECULE compared to 1/12th of the mass of one atom of carbon-12

Question 22

What is the formulae for relative atomic mass

Answer 22

Isotopic mass x % abundance
________________________________
100/ whatever the % abundance sum is

Question 23

How do you determine the relative atomic mass

Answer 23

• using mass spectrometry

Question 24

How does a mass spectra work

Answer 24

1) sample is placed in the mass spectrometer
2) sample is vaporised and ionised to be ions (positively charged)
3) ions are accelerated where the heavier ions (based on isotopic mass) are slower and less deflected
4) ions are detected by mass spectrum as a mass charge ratio

Question 25

State the charge of Zn

Answer 25

2+

Question 26

State the charge of Ag

Answer 26

1+

Question 27

State the charge of NH4

Answer 27

1+

Question 28

State the charge of CO3

Answer 28

2-

Question 29

State the charge of NO3

Answer 29

1-

Question 30

State the charge of SO4

Answer 30

2-

Question 31

State the charge of OH

Answer 31

1-

Question 32

State the charge of Cr2O7

Answer 32

2-

Question 33

State the charge of PO4

Answer 33

3-

Question 34

State the charge of HCO3

Answer 34

1-

Question 35

State the charge of MnO4

Answer 35

1-

Question 36

What state compound do metals + metal oxides always produce

Answer 36

- Solids

Question 37

what is meant by the term weighted mean mass

Answer 37

-the average mass of an element’s isotopes, taking into account the abundance of each isotope