C2 - The Periodic Table

Question 1

How did the periodic table develop?

Answer 1

• Chemists tried to classify the elements, they arranged them in order in which similar elements were grouped together.

Question 2

Why is the periodic table so named?

Answer 2

• Regular repeating of patterns in the properties of elements.

Question 3

Features of Mendeleev’s periodic table.

Answer 3

• Left gaps for unnamed elements.

- When they were discovered, the scientific community accepted his periodic table.

Question 4

What is an atomic (proton) number?

Answer 4

• Determines its position in the periodic table.
• Bottom number of an element in the periodic table moving from left to right.
• How many protons the elements will have, therefore the same amount of electrons.

Question 5

What does the amount of electrons determine in an element?

Answer 5

• Electrons in the outermost shell (highest energy level) determines its chemical properties.

Question 6

What does the group number of an element equal to in the actual element?

Answer 6

• The amount of electron it has on the outermost shell.

Question 7

Do atoms of metals tend to lose of gain electrons?

Answer 7

Lose electrons.

Question 8

Do atoms of non-metals tend to lose or gain electrons?

Answer 8

Gain electrons.

Question 9

Why are noble gases in group 0 very un-reactive?

Answer 9

• Due to their stable electron arrangements.

Question 10

What are the metal in group 1 known as?

Answer 10

• The alkali metals.

Question 11

What happens to the metals boiling and melting points as you go down group 1?

Answer 11

• They decrease.

Question 12

Do all the metals in group 1 react with water and what happens if it does?

Answer 12

• Yes.

- They produce hydrogen and an alkaline solution called sodium hydroxide.

Question 13

What are the ions group 1 metals form?

Answer 13

• They create 1+ ions in reaction to make ionic compounds. - Generally white and dissolve in water giving colourless solutions.

Question 14

What happens to the reactivity of the metals as you got down the group 1?

Answer 14

The reactivity increases as you go down the group.

Question 15

What ions do the elements in group 7 produce (halogens)?

Answer 15

• 1- ions in their ionic compounds with metals.

Question 16

What compounds do the halogens form?

Answer 16

• Covalent compounds by sharing electrons with other non-metals.

Question 17

How can a more reactive halogen displace a lower reactive halogen?

Answer 17

• From a solution of one of its salts.

Question 18

What happens to the reactivity as you go down the halogens?

Answer 18

• It decreases as you go down the group.

Question 19

How can you explain trends in reactivity?

Answer 19

• You can go down a group in the periodic table in terms of the attraction between electrons in the outermost shell and the nucleus.

Question 20

What does the electrostatic attraction depend on?

Answer 20

• Distance between outermost electrons and the nucleus.
• Number of occupied inner shells (energy levels), which provide a shielding effect.
• Size of the positive charge on the nucleus.

Question 21

How do you decide if it is easy for atoms to lose or gain electrons from their outermost shells?

Answer 21

• The three factors on electrostatic attraction must be taken into account.
• The increased nuclear charge due to extra charge in the nucleus. Going down a group is outweighing the 2 other factors.

Question 22

Gain/Loss of electrons in a larger atom.

Answer 22

• Easier to lose going down a group.

- Harder for them to gain going up a group.