Unit 1, Topic 2-Atomic Structure

Question 1

The periodic table is a useful way of arranging elements. How does this arrangement help chemists?

Answer 1

Elements with similar physical and chemical properties are placed in the same group. So there are trends across periods.

Question 2

How can an element be tested to determine if it is a metal or non-metal?

Answer 2

You can test to see if the element conducts electricity. Metals do, non-metals don’t. (apart from graphite, one form of carbon)

Question 3

What is a vertical column of elements called in the periodic table?

Answer 3

A group

Question 4

What is a horizontal row of elements called in the periodic table?

Answer 4

A period

Question 5

In what way are elements in the same group similar?

Answer 5

They have similar chemical properties, they have the same amount of electrons in the outer shell. This causes them to react similarly to different substances.

Question 6

What is the name of group 1?

Answer 6

Alkali metals

Question 7

What is the name of group 7?

Answer 7

The halogens

Question 8

What is the name of group 8?

Answer 8

Noble gases

Question 9

Area between 2&3?

Answer 9

Transitional metals

Question 10

Name the group which contains very reactive metals.

Answer 10

Alkali metals

Question 11

Name the group which contains very reactive non-metals.

Answer 11

Halogens

Question 12

Name the group which contains very unreactive non-metals

Answer 12

Noble gases

Question 13

Where can you locate electrons in the atom?

Answer 13

The shell

Question 14

Where can you locate neutrons in the atom?

Answer 14

The nucleus

Question 15

Where can you locate protons in the atom?

Answer 15

The nucleus

Question 16

What type of particle is every element made of?

Answer 16

atoms

Question 17

What are the three sub-atomic particles?

Answer 17

Protons, neutrons, electrons

Question 18

What is at the centre of every atom and what type of subatomic particles does it contain?

Answer 18

The nucleus, it contains protons and neutrons.

Question 19

What are the charges on each of the sub-atomic particles?

Answer 19

Protons +1
Electrons -1
Neutron 0

Question 20

Why are atoms neutral?

Answer 20

because they always contain equal number of positive protons and negative electrons.

Question 21

What mass does each of the sub-atomic particles have? (amu)

Answer 21

Proton 1
Neutron 1
Electron 0 (very small insignificant mass)

Question 22

What is used to put the elements in order in the periodic table?

Answer 22

In order of atomic number

Question 23

What is the atomic number?

Answer 23

The amount of protons in the nucleus

Question 24

What is the mass number?

Answer 24

The number of protons plus neutrons in the nucleus of an atom.

Question 25

How do you write nuclide notation?

Answer 25

mass number ---> 35 Cl atomic number---> 17

Question 26

How can the number of neutrons in an atom be calculated?

Answer 26

Mass number minus atomic number.

Question 27

What is the maximum number of electrons that each of the three electron shells hold?

Answer 27

2,8,8

Question 28

What can be said about the number of electrons in the outer shell of the atoms of elements in the same group of the periodic table?

Answer 28

They have the same number of electrons in their outer shell.

Question 29

Know how to write the electron arrangement for any of the first 20 elements

Answer 29

eg Chlorine 2,8,7

Question 30

What are isotopes?

Answer 30

Atoms of the same element with different mass numbers (i.e different number of neutrons in the nucleus)

Question 31

Do most elements have isotopes?

Answer 31

yes.

Question 32

What is the relative atomic mass of an element?

Answer 32

The average mass of an element taking into account the proportion/abundance of each isotope present.

Question 33

Chlorine has an RAM (relative atomic mass) of 35.5. There are two isotopes of chlorine, chlorine-35 and chlorine-37. Which is more abundant/common?

Answer 33

Chlorine-35 is more abundant as the RAM value is closer in value to he mass of this isotope.