3.1 Periodic trends

Front

Which of the following is FALSE about periodic table? Options: Group is vertical column, Period is horizontal row, s block are elements with electrons in s sublevel., Elements in same group have same number of electrons

Back

Elements in same group have same number of electrons

Front

Which of the following DOES NOT affect the ionization energy? Options: Distance from nucleus, Nuclear charge, Electron - electron repulsion, Electronegativity

Back

Electronegativity

Front

Why does ionization increase across a period?

Back

Nuclear charge increases due to an increase in proton number.

Front

Ionization decreases down the group because of the following statement except: the distance from nucleus increases, greater electron electron repulsion, nuclear charge increases due to increase in proton number, more electrons in the inner shell causing shielding effect

Back

nuclear charge increases due to increase in proton number

Front

Why does ionization energy decrease from Be (1s²2s²) to B (1s²2s²2p¹)? Options: increase in nuclear charge from Be to B, valence electron is further away from nucleus, valence electron in p sublevel, further away from nucleus, greater electron electron repulsion.

Back

valence electron in p sublevel, further away from nucleus

Front

Ionization energy decreases from N (1s²2s²2p³) to O (1s²2s²2p⁴) due to:

• increase in nuclear charge from N to O
• valence electron is further away from nucleus
• valence electron in 2p sublevel, further away from nucleus
• greater electron electron repulsion in same 2p orbital

Back

greater electron electron repulsion in same 2p orbital

Front

Ionization energy for period 3 is less than period 2 due to

Back

valence electron for period 3 is further away from nucleus

Front

Atomic radius decreases across period 2 and 3 because

Back

increase in nuclear charge across period 2 and 3

Front

Why do positive Na⁺ ions have a smaller ionic radius than Na atoms?

Back

decrease in number of shell for Na⁺ ion

Front

Why is the ionic radius for S^2- ion greater than S atom?

Back

Increase in electron-electron repulsion due to inner electron