B1 Atomic Structure

Question 1

Define element

Answer 1

a substance that cannot be broken down into simpler substances by chemical methods

Question 2

Define atom

Answer 2

the smallest particle of an element which still retain the chemical properties of the element

Question 3

Describe the structure of an atom (mentioning the structure of its subatomic particles)

Answer 3

Each atom has a central nucleus (containing protons and neutrons) surrounded by electrons moving in shells/energy levels.

Question 4

What is the relative charge of a proton

Answer 4

+1

Question 5

What is the relative charge of an electron

Answer 5

-1

Question 6

What is the relative charge of a neutron

Answer 6

0

Question 7

What is the relative mass of a proton

Answer 7

1

Question 8

What is the relative mass of a neutron

Answer 8

1

Question 9

What is the relative mass of an electron

Answer 9

0.0005

Question 10

Where can you find the protons in an atom

Answer 10

nucleus

Question 11

Where can you find the neutrons in an atom

Answer 11

nucleus

Question 12

Where can you find the electrons in the atom

Answer 12

electron shell (orbital)

Question 13

Where can you find most of the mass of an atom

Answer 13

nucleus

Question 14

Define atomic number

Answer 14

the number of protons in an atom (number of electrons = number of protons)

Question 15

Define mass number

Answer 15

the total number of protons and neutrons in an

atom

Question 16

What letter represents atomic number

Answer 16

A

Question 17

What letter represents atomic mass

Answer 17

Z

Question 18

What state of charge are all atoms in

Answer 18

Since number of electrons = number of protons, atoms are neutral (no charge)

Question 19

What does x represent in standard notation for atoms

Answer 19

Chemical symbol of element

Question 20

How many electrons are in the outer shell for the first four energy levels

Answer 20

2, 8 (10), 8 (18), 8 (26)

Question 21

Define isotope

Answer 21

atoms of an element with the same number of protons but different numbers of neutrons
(hence having different mass numbers)

Question 22

Define relative atomic mass

Answer 22

average mass of one atom of the element when compared with 1/12 the mass of an atom of carbon-12

Question 23

What is the relative atomic mass of isotopes 24Mg, 25Mg and 26Mg if they’re in the ratio of 79:10:11

Answer 23

(79/100 x 24) + (10/100 x 25) + 11/100 x 26) = 24.32

Question 24

How do you calculate percentage abundance

Answer 24

number of atoms of a given isotope/total number of atoms of all isotopes x 100

Question 25

How do we determine isotope mass/relative abundance of isotopes

Answer 25

percentage abundance and the masses of the isotopes are determined experimentally using a mass spectrometer.

Question 26

What is the mass spectrum

Answer 26

a plot of the relative abundance of the charged particle versus the ratio of mass/charge (m/z).

Question 27

Describe what the electronic configuration of the first 20 elements are

Answer 27

Hydrogen = 1
Helium = 2
Lithium = 2,1
Beryllium = 2,2
Boron = 2,3
Carbon = 2,4
Nitrogen = 2,5 
Oxygen = 2,6
Fluorine = 2,7
Neon = 2,8
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