1.1: Atomic Structure

Question 1

what is the name of the sub-atomic particles

Answer 1

-protons
-neutrons
- electrons

Question 2

what is the relative charges of the subatomic particles?

Answer 2

proton: +1
neutron: 0
electron: -1

Question 3

what is the relative mass of the subatomic particles?

Answer 3

proton: 1
neutron: 1
electron: 1/1840

Question 4

where are the particles in the atom?

Answer 4

in the nucleus, the protons and neutrons are found. The electrons orbit the nucleus in shells

Question 5

How do you work out the number of protons in an atom?

Answer 5

By using the atomic number or proton number on the periodic table

Question 6

How do you work out the number of electrons in an atom?

Answer 6

Electrons have the same number of protons in a neutrally charged atom (atomic number)

Question 7

How do you work out the number of neutrons in an atom?

Answer 7

By working out the mass number, which is the number of protons + the number of neutrons
- or the mass no. - atomic no.

Question 8

What is an Ion?

Answer 8

When an atom loses or gains one or more electrons from the outer shell, which results in a net positive or negative charge on the particle.

Question 9

What are isotopes?

Answer 9

Atoms of the same element (same number of protons) but a different number of neutrons (mass number)

Question 9

How can you use the periodic table to deduce ions?

Answer 9

By seeing which row in the periodic table the elements are

Question 10

what are the qualities of isotopes

Answer 10

They have the same chemical properties because they have the same number of electrons in the outer shell

Question 11

What is the relative isotopic mass?

Answer 11

The mass of an atom of an isotope compared to 1/12th of the mass of an atom of carbon -12

Question 12

What is the definition of the relative atomic mass (Ar) ?

Answer 12

The average mass of an atom of an element compared to 1/12th of the mass of an atom of carbon 12.

Question 13

How do you calculate the relative atomic mass?

Answer 13

(mass of isotope 1 x % of abundance) + (mass of isotope 2 x % of abundance) / 100

Question 14

What is the electronic configuration?

Answer 14

The term to describe where and how the electrons are arranged

Question 15

What do electrons do for the elements?

Answer 15

Determine the chemical reactivity and how they react with other elements.

Question 16

What are shells?

Answer 16

Electrons are arranged into principle quantum shells. These are major energy levels and follow a pattern.

Question 17

How many electrons do each quantum shell contain?

Answer 17

shell 1 - 2
shell 2 - 8
shell 3 - 18
shell 4 - 32

Question 18

what letters are assigned to sub-shells?

Answer 18

s, p, d, f

Question 19

What is sub-shells made up of?

Answer 19

Atomic orbitals of the same type

Question 20

what is an orbital?

Answer 20

Orbitals are defined as a region of space with an atom that contains up to 2 electron of opposite spin

Question 21

What is the sub-shells equal to?

Answer 21

The number of the shell. (For example: Shell 1 has 1 sub-shell)

Question 22

What shape is s-orbitals?

Answer 22

spherical

Question 23

How many orbitals are there in a p-orbital and what shape are they?

Answer 23

3 orbitals, dumbbell shaped

Question 24

What is the Aufbau principle?

Answer 24

Within each quantum level the sub-shells also fill into the lowest available orbital

Question 25

What order to the sub shells fill in?

Answer 25

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, etc.

Question 26

What is the rule with 4s and 3d sub-shells?

Answer 26

The 4s is filled before the 3d because the 4s has lower energy

Question 27

What is Hund’s Rule?

Answer 27

Orbitals of the same energy will be filled singly before being paired up - this is important for electrons in the p-subshell and d-subshell

Question 28

What are the exceptions to the Aufbau principle?

Answer 28

chromium and copper. In these 2 elements, the 3d sub shell is half-filled and fully-filled which fully stabilises the atoms.

Question 29

What happens with ions?

Answer 29

Electrons are lost or gained. They are added to the outer most energy level (shell)

Question 30

What is the rule for transition elements?

Answer 30

4s electrons are lost first.

Question 31

What is 1st Ionisation Energy?

Answer 31

The energy required to remove one mole of electrons from one mole of gaseous atoms

Question 32

What is 1st Ionisation Energy as an equation?

Answer 32

X(g) –> X+ (g) + e-

Question 33

What factors will affect the amount of energy needed to remove the outermost electron from an atom? (Number of protons)

Answer 33

• The strength of attraction between the nucleus and the outer electron.
• The more protons there are in the nucleus (nuclear charge) the greater attraction between the nucleus and the outermost electron. This means more energy is needed to remove the electron.

Question 34

What factors will affect the amount of energy needed to remove the outermost electron from an atom? (number of shells)

Answer 34

• The more shells there are the further the outermost electron is from the nucleus, and the more shells there are in between nucleus and the outermost electron.
• Electrons in the shells in-between the nucleus and outermost electron reduces the attraction of the nucleus to outermost electron called shielding.
• The more shells the more shielding.
  The greater the shielding, the weaker the nuclear attraction and less energy needed to remove electron.

Question 35

What is a reason for ionisation energy decreasing? (sub-shells)

Answer 35

There is a pair of electrons in a sub-shell, which means that they are repelling each other making it easier to lose an outer shell electron.