Atomic structure and the periodic table

Question 1

Thompson discovered the electron(1988) then created what?

Answer 1

The plum pudding model

Question 2

What is the plum pudding model?

Answer 2

The plum pudding model is a ball of positive charge with electrons embedded within it

Question 3

What is the gold foil experiment?

Answer 3

Rutherford directed alpha particles at a thin sheet of gold to test the plum pudding model

Question 4

What did the gold foil experiment prove?

Answer 4

.Most alpha particles went straight through proving the atom is mostly empty space
.Some particles deflected straight back proving the nucleus

Question 5

What is the Nuclear model

Answer 5

In Rutherford’s the atom consists of mainly empty space with the nucleus at the centre and electrons orbiting around it

Question 6

What is the Bohr Model?

Answer 6

1913, Niels Bohr proposed that electrons orbit the nucleus in fixed shells and the nucleus can be divided into smaller parts (proton)

Question 7

Why did Mendeleev leaves gaps in his periodic table?

Answer 7

For elements that are undiscovered

Question 8

How did Mendeleev organise elements?

Answer 8

In increasing atomic weight

Question 9

How is the modern periodic table arranged?

Answer 9

It is arranged in increasing atomic number

Question 10

Elements that react by losing electrons to form positive ions are called?

Answer 10

Metals

Question 11

Elements that react by gaining electrons to form negative ions are called?

Answer 11

Non-metals

Question 12

What does increasing atomic size do to the attraction of the nucleus?

Answer 12

Increasing atomic size weakens attraction to the nucleus

Question 13

For Metals what is the relationship between reactivity and atomic size?

Answer 13

Reactivity increases as atomic size increases

Question 14

For Non-metals what is the relationship between reactivity and atomic size?

Answer 14

Reactivity decreases as atomic size increases

Question 15

Properties of Group 0 (Noble gases)

Answer 15

.Low melting and boiling points
.Are monoatomic
.Full outer shell
.Extremely stable electronic configuration making them unreactive and inert(unactive)
.Boiling point increases down group due to increase in relative atomic mass
.Are non-metals

Question 16

Properties of group 1 (Alkali metals)

Answer 16

.1 outer shell electron
.Low melting and boiling point that decreases down the group
.Low density

Question 17

Properties of group 7 (Halogens)

Answer 17

.7 outer shell electrons
.Diatomic
.Reactivity decreases down group due to increasing atomic size

Question 18

How do you calculate relative formula mass(Mr)?

Answer 18

You have to add up the relative atomic masses of all the atoms present in the formula.