1. CHEMISTRY DEPARTMENT WAID ACADEMY Trends in the Periodic Table

2. The difference in atomic size of sodium and chlorine is mainly due to the difference in the 1.number of electrons. 2.number of protons. 3.number of neutrons. 4.mass of each atom. 25

3. In which molecule will the chlorine atom carry a partial positive charge? 25 1.Cl-Br 2.Cl-Cl 3.Cl-I 4.Cl-F

4. Which description shows the trends in the electronegativity values of elements in the Periodic Table? 30 1.Decrease across a period and increase down a group. 2.Increase across a period and increase down a group. 3.Increase across a period and decrease down a group. 4.Decrease across a period and decrease down a group.

5. Which of the following chlorides is likely to have the most ionic character? 30 1.LiCl 2.CsCl 3.BeCl 2 4.CaCl 2

6. Which equation represents the first ionisation energy of a diatomic element, X 2 ? 30 1.½ X 2 (s)  X+(g) + e - 2.½ X 2 (s) + e-  X-(g) 3.X(g)  X + (g) + e - 4.X(g) + e -  X - (g)

7. Which of the following elements has the greatest electronegativity? 30 1.Fluorine 2.Caesium 3.Iodine 4.Sodium

8. As the relative atomic mass in the halogens increases 30 1.the density decreases. 2.the boiling point increases. 3.the first ionisation increases. 4.the atomic size decreases.

9. Which of the following elements would require the most energy to convert one mole of gaseous atoms into gaseous ions each carrying two positive charges? 30 1.Scandium 2.Titanium 3.Vanadium 4.Chromium

10. On descending the halogen group of the Periodic Table, the 30 1.attracting power for bonding electrons increases. 2.ionisation energy increases. 3.nuclear charge increases. 4.reactivity increases.

11. Which of the processes represents the second ionisation energy of magnesium? 30 1.Mg + (g)  Mg 2+ (g) + e - 2.Mg(g)  Mg 2+ (g) + 2e - 3.Mg(s)  Mg 2+ (g) + 2e - 4.Mg + (s)  Mg 2+ (g) + e -