Question 1
Which of the following best describes the trend in atomic size as you move from left to right across a period in the periodic table?
A. Increases steadily
B. Decreases steadily
C. Remains constant
D. First increases, then decreases
Question 2
Which factor primarily affects the electronegativity of an element?
A. Number of electron shells
B. Number of valence electrons
C. Distance of valence electrons from the nucleus
D. Number of neutrons
Question 3
Which of the following elements has the highest electronegativity?
A. Sodium
B. Chlorine
C. Iron
D. Neon
Question 4
How does atomic size change as you move down a group in the periodic table?
A. Increases
B. Decreases
C. Remains constant
D. First decreases, then increases
Question 5
Which of the following best describes the trend in ionisation energy as you move from left to right across a period?
A. Increases
B. Decreases
C. Remains constant
D. First decreases, then increases
Question 6
a) Define atomic size and explain the factors that influence it. [3]
b) How does atomic size change as you move from left to right across a period in the periodic table? [2]
Question 7
a) Define electronegativity and mention the scale commonly used to measure it. [2]
b) Describe the trend in electronegativity as you move down a group in the periodic table. [3]
Question 8
a) What are transition metals, and how do they differ from main group elements in terms of their electron configuration? [3]
b) Why are many transition metals important catalysts in industrial processes? [2]
Question 9
a) Describe the general trend in atomic size as you move from the top to the bottom of a group in the periodic table. [2]
b) Explain the underlying reason for this trend in atomic size. [3]
c) How does this trend affect the reactivity of alkali metals? [2]
Question 10
a) Define ionisation energy and state its unit of measurement. [2]
b) Describe the trend in first ionisation energy as you move from left to right across a period. [3]
c) Explain the reason for the observed trend in part b. [2]
Question 11
Which of the following elements would have the lowest ionisation energy?
A. Helium
B. Lithium
C. Oxygen
D. Fluorine
Question 12
Which of the following is a key factor affecting electron affinity?
A. Atomic size
B. Number of isotopes
C. Melting point
D. Density
Question 13
How does electron affinity change as you move down a group in the periodic table?
A. Increases
B. Decreases
C. Remains constant
D. First increases, then decreases
Question 14
Which of the following elements would most likely have the highest electron affinity?
A. Potassium
B. Carbon
C. Neon
D. Chlorine
Question 15
Which of the following best describes the trend in metallic character as you move from left to right across a period?
A. Increases
B. Decreases
C. Remains constant
D. First increases, then decreases
Question 16
a) What is electronegativity, and how is it different from electron affinity? [3]
b) Which element in the periodic table is considered to have the highest electronegativity? [1]
c) Explain the implications of high electronegativity on the type of bonding an element will predominantly form. [3]
Question 17
a) Describe the trend in metallic character as you move from left to right across a period. [2]
b) How does this trend relate to ionisation energy? [3]
c) Why do elements on the far right of the periodic table, like noble gases, not exhibit typical metallic properties? [2]
Question 18
a) Define atomic radius and explain how it is typically measured. [2]
b) Predict the atomic radius trend as you move from the top to the bottom of Group 1 (alkali metals) in the periodic table. [2]
c) Contrast this with the trend in atomic radius as you move from left to right across Period 3. [3]
d) Provide a reason for the difference in trends observed in parts b and c. [3]
Question 19
a) What is meant by the term "electronegativity"? [2]
b) Using the Pauling scale, which element is considered the least electronegative? [2]
c) How does electronegativity influence the type of bond formed between two atoms? [3]
d) Predict the type of bond that would form between chlorine (Cl) and bromine (Br), and justify your answer. [3]
Question 20
a) Define ionisation energy and explain its significance in understanding atomic properties. [3]
b) Why does ionisation energy generally increase as you move from left to right across a period? [3]
c) Predict the trend in ionisation energy as you move down Group 17 (halogens). [2]
d) How does the ionisation energy of an element relate to its metallic or non-metallic character? [2]