Chemistry 9th Chap 4 : Topic 5 - Maryam Publications

Chemistry Chapter 4 : Topic 5

Periodic Property Trends

1 / 25

In a period, as you move from left to right across the periodic table, the atomic radius generally decreases. Which statement best explains this trend?

A) Nuclear charge increases while electrons are added to the same shell, pulling them closer

B) New shells are added, increasing size

C) Electron shielding increases significantly across the period

D) Atomic mass decreases, reducing size

2 / 25

Element X is located on the left side of the periodic table, while Element Y is on the right side of the same period. Which comparison is correct?

A) X has greater non-metallic character than Y.

B) Y has larger atomic radius than X.

C) Y has higher ionization energy than X.

D) X has higher electronegativity than Y.

3 / 25

Which statement correctly describes the trend of electronegativity in the periodic table?

A) It increases down a group and decreases across a period

B) It remains constant in all directions

C) It decreases both across a period and down a group

D) It increases across a period and decreases down a group

4 / 25

Element A has low ionization energy and easily loses electrons, while Element B has high ionization energy and strongly attracts electrons. What can be concluded?

A) A is a non-metal, B is a metal

B) A is a metal, B is a non-metal

C) Both are non-metals

D) Both are metals

5 / 25

Why does atomic radius increase down a group in the periodic table?

A) New electron shells are added with increased distance from nucleus

B) Ionization energy increases

C) Electrons are removed from outer shell

D) Nuclear charge increases rapidly

6 / 25

Which element is expected to have the highest electronegativity?

A) Sodium (Na)

B) Chlorine (Cl)

C) Potassium (K)

D) Magnesium (Mg)

7 / 25

A student observes that element P reacts vigorously with water, while element Q reacts slowly. If both are in the same group, what is most likely true?

A) Both have same atomic size

B) Both are in different groups

C) Q is below P in the group

D) P is below Q in the group

8 / 25

Which trend correctly describes ionization energy across a period?

A) Decreases due to increasing atomic size

B) Increases due to increasing nuclear charge

C) Remains constant

D) Random variation

9 / 25

Which statement best explains why metals are found on the left side of the periodic table?

A) They easily gain electrons

B) They have small atomic radius

C) They have high electronegativity

D) They have low ionization energy and lose electrons easily

10 / 25

Element X has higher metallic character than Element Y in the same period. What is true?

A) X is located on the left side of Y.

B) Y has larger atomic radius.

C) X has higher electronegativity.

D) X is located on the right side of Y.

11 / 25

Which factor mainly affects atomic radius across a period?

A) Number of shells

B) Mass number

C) Nuclear charge

D) Neutron count

12 / 25

Why do noble gases generally have very low reactivity?

A) They have low atomic mass

B) Their outer shells are complete and stable

C) They easily lose electrons

D) They have incomplete outer shells

13 / 25

Which property generally increases down Group 1 elements?

A) Non-metallic character

B) Ionization energy

C) Reactivity with water

D) Electronegativity

14 / 25

Why does electronegativity decrease down a group?

A) Nuclear charge increases

B) Atomic radius decreases

C) Number of protons decreases

D) Shielding effect increases and reduces nuclear attraction

15 / 25

Which element has the largest atomic radius?

A) Fluorine

B) Potassium

C) Lithium

D) Oxygen

16 / 25

A student compares two elements: one has high density and high melting point, the other has low density and low melting point. What can be inferred?

A) Both are metals

B) Both are non-metals

C) First is non-metal, second is metal

D) First is metal, second is non-metal

17 / 25

Which trend is correct for metallic character across a period?

A) Remains constant

B) Decreases left to right

C) Increases left to right

D) First increases then decreases

18 / 25

Which element would most likely have the highest ionization energy?

A) Chlorine

B) Sodium

C) Aluminum

D) Argon

19 / 25

Why does reactivity of non-metals increase across a period?

A) Atomic size increases

B) Shielding increases

C) Electronegativity decreases

D) Electronegativity increases

20 / 25

Which statement about density trend is generally correct?

A) Density increases across a period only

B) Density decreases down all groups

C) Density is unrelated to periodic trends

D) Density increases for most elements down a group

21 / 25

Element A has atomic number 11 and Element B has atomic number 17. Which comparison is correct?

A) B has larger atomic radius

B) A is more non-metallic

C) A has higher electronegativity

D) B has higher ionization energy

22 / 25

What is the reason for decreasing atomic radius across a period?

A) Increase in shielding effect

B) Addition of shells

C) Increase in nuclear charge without new shells

D) Loss of protons

23 / 25

Which property is inversely related to atomic radius in a period?

A) Atomic mass

B) Number of neutrons

C) Ionization energy

D) Density always

24 / 25

Why is fluorine the most electronegative element?

A) It has weakest nuclear charge.

B) It has largest atomic size.

C) It has full outer shell.

D) It has small size and high nuclear attraction.

25 / 25

Which best explains periodic trends?

A) Based on atomic number and electron configuration

B) Based on atomic mass only

C) Based on density only

D) Random arrangement of elements

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