Atomic Structure And Perodic Table | Topic 1

Question 1

Name the subatomic particles in an atom

Answer 1

Proton, neutrons and electrons

Question 2

state the relative charges of such particles:
Protons, neutron and electron

Answer 2

1,0, -1

Question 3

Define atomic number

Answer 3

is the number of protons in the atom

Question 4

Define mass number

Answer 4

The sum of the number of protons and neutrons in the atom

Question 5

Define isotope

Answer 5

atoms of the same element that contain the same number of protons and electrons but a different number of neutrons.

Question 6

What is relative atomic mass?

Answer 6

is the average mass of an atom of an element relative to one twelfth of the mass of an atom of carbon-12

Question 7

What’s is relative isotopic mass?

Answer 7

is the mass of an atom of an element relative to one twelfth of the mass of an atom of carbon-12.

Question 8

Describe how mass spectrometry works and information you can obtain

Answer 8

used to identify different isotopes and find the overall relative atomic mass of an element. This form of mass spectrometry records the time it takes for ions of each isotope to reach a detector.

Question 9

What is relative molecular mass?

Answer 9

is the average mass of a molecule relative to one twelfth of the mass of an atom of carbon-12. It is the sum of the relative atomic masses of each atom within the molecule.

Question 10

What is relative formula mass?

Answer 10

is the relative mass used for giant covalent compounds or ionic compounds. An example of a giant covalent or ionic compound is Mg(OH)2.

Question 11

What’s the s orbital shape?

Answer 11

Sphere

Question 12

What’s the p orbital shape

Answer 12

Dumbell

Question 13

How many electrons can the s orbital , p orbital, d orbital have?

Answer 13

2,6,10

Question 14

What’s the first ionisation energy

Answer 14

Energy required to remove one mole of electrons from one mole of gaseous atoms

Question 15

State and explain the trend in the first ionisation energies acrossthe period.

Answer 15

They increase becausethe nuclear charge increases and the shielding is the same throughout. The atomic radius decreases

Question 16

State and explain the trend in first ionisation energies as we go down a group in periodic table

Answer 16

The less attracted to the nucleus. first ionisation energies decrease because whilst the nuclear charge increase the shielding increase due Tu more shells.
As the atomic radius increases the outer shell electrons are less attracted to the nucleus.

Question 17

Which atom in Group 6 has a higher ionisation energy sulphur or oxygen.

Answer 17

The 2p electron is closer to nucleus
Then sulphur 3p