Question 1:
Give two examples of Group 1 elements.
Answer:
Lithium and rubidium (any Group 1 element)
Give two examples of Group 1 elements.
Answer:
Lithium and rubidium (any Group 1 element)
Question 2:
Table 4.5 shows the electron arrangement for elements X, Y and Z.
(a) Give two differences in physical properties between elements X, Y and Z.
(b) Element X reacts with oxygen when heated. Write the chemical equation for this reaction.
(c) Arrange the reactivity of elements X, Y and Z in ascending order. Explain the difference in reactivity.
Answer:
(a)
• The melting point and boiling point of X are the highest, followed with Y and Z.
• The size of atom Z is the largest, followed with Y and X
(b) 4X(s) + O2(g) → 2X2O(s)
(c) Reactivity in increasing order: X, Y, Z
Metal Z is the most reactive, followed with metals Y and X. The reactivity of Group 1 metals increases when going down the group because the size of atoms increases. Hence it is easier for the atom to donate the valence electron that is further away from the nucleus.
Table 4.5 shows the electron arrangement for elements X, Y and Z.
(a) Give two differences in physical properties between elements X, Y and Z.
(b) Element X reacts with oxygen when heated. Write the chemical equation for this reaction.
(c) Arrange the reactivity of elements X, Y and Z in ascending order. Explain the difference in reactivity.
Answer:
(a)
• The melting point and boiling point of X are the highest, followed with Y and Z.
• The size of atom Z is the largest, followed with Y and X
(b) 4X(s) + O2(g) → 2X2O(s)
(c) Reactivity in increasing order: X, Y, Z
Metal Z is the most reactive, followed with metals Y and X. The reactivity of Group 1 metals increases when going down the group because the size of atoms increases. Hence it is easier for the atom to donate the valence electron that is further away from the nucleus.