Chemistry 9th Chap 4 : Topic 7 - Maryam Publications

Chemistry Chapter 4 : Topic 7

Group Property Prediction

1 / 15

An element X is placed in Group 1 of the periodic table. A student predicts that X will have a low ionization energy, will react vigorously with water, and will form a stable + 1 ion by losing its outermost electron. Which statement best justifies this prediction?

A) Elements in Group 1 have one valence electron that is loosely held, making electron loss easy.

B) Elements in Group 1 are inert due to full outer shells.

C) Elements in Group 1 have two valence electrons and form + 2 ions by gaining electrons.

D) Elements in Group 1 are non-metals that tend to gain electrons to complete octet.

2 / 15

An unknown element is placed in Group 17. A student predicts that it will have high electronegativity, will form negative ions, and will likely exist as a diatomic molecule. Which property most strongly supports this prediction?

A) Metallic bonding with delocalized electrons

B) High nuclear attraction for gaining one electron to complete octet

C) Presence of one valence electron

D) Strong tendency to lose electrons

3 / 15

An element is located in Group 18 of the periodic table. A student predicts it will be chemically unreactive, monatomic in nature, and have a full outer electron shell. What is the best explanation for this prediction?

A) It has incomplete valence shell and easily forms bonds.

B) It readily loses electrons due to low ionization energy.

C) It has high tendency to form ionic bonds.

D) It has complete valence shell making it stable and inert.

4 / 15

A student analyzes an element in Group 2 and predicts it will form basic oxides, show moderate reactivity, and produce + 2 ions in chemical reactions. Which reasoning supports this prediction?

A) The element behaves like a non-metal.

B) The element has completely filled outer shell.

C) The element has two valence electrons that are easily lost.

D) The element has seven valence electrons that are easily gained.

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An element is predicted to be a transition metal. The student expects it to show variable oxidation states, form colored compounds, and act as a catalyst. Which feature mainly explains this behavior?

A) Low electronegativity and non-metallic nature

B) Participation of d-orbitals in bonding

C) Lack of valence electrons

D) Presence of completely filled outer shell

6 / 15

An element is located in the halogen group. A student predicts that it will form salts with metals and show decreasing reactivity down the group. Which statement best explains this trend?

A) Atomic size decreases and attraction increases down the group

B) Atomic size increases and electron gain becomes more difficult down the group

C) Valence electrons increase down the group

D) Nuclear charge increases sharply causing instability

7 / 15

An element is placed in Group 1 and the student predicts its reactivity will increase as you move down the group. Which explanation best supports this prediction?

A) Nuclear attraction increases down the group

B) Number of protons decreases down the group

C) Atomic radius decreases down the group

D) Outer electron becomes farther from nucleus and is lost more easily

8 / 15

An element is identified as a lanthanide. A student predicts that it will be a silvery metal, form + 3 ions commonly, and be used in alloys and magnets. Which property mainly leads to this prediction?

A) Gaseous state at room temperature

B) Complete octet configuration

C) High electronegativity

D) Filling of 4f orbitals and metallic nature

9 / 15

An element is predicted to be radioactive and unstable, belonging to the actinide series. It is also expected to form multiple oxidation states. Which characteristic supports this prediction?

A) Involvement of 5f orbitals and unstable nuclei

B) High electronegativity and non-metallic nature

C) Complete valence shell stability

D) Presence of only s-orbital electrons

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A student predicts that an element in the same group as fluorine will be more reactive than chlorine. Which reasoning is correct?

A) Fluorine has larger atomic size than chlorine.

B) Fluorine has stronger nuclear attraction due to smaller atomic size.

C) Fluorine has more electron shells than chlorine.

D) Chlorine has higher electronegativity than fluorine.

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An element is predicted to have metallic bonding, high electrical conductivity, and form alloys. It is located in the transition series. Which feature best explains these properties?

A) Lack of valence electrons

B) Complete valence shell stability

C) Presence of free-moving delocalized electrons in d-orbitals

D) Strong tendency to form covalent molecules

12 / 15

An element is placed in Group 2. A student predicts that it will react less violently with water than Group 1 elements. Which explanation is correct?

A) It has a full outer shell.

B) It has one valence electron.

C) It has no valence electrons.

D) It has two valence electrons which require more energy to remove.

13 / 15

An element is predicted to form ionic bonds easily with metals due to high electronegativity and strong electron gain tendency. Which group does it most likely belong to?

A) Noble gases

B) Transition metals

C) Halogens

D) Alkali metals

14 / 15

A student predicts that noble gases will not participate in chemical reactions under normal conditions. Which explanation best supports this?

A) They have one valence electron.

B) They easily form ions.

C) They have full outer electron shells.

D) They have high metallic character.

15 / 15

An element is expected to show increasing metallic character as it moves down a group. Which reason explains this trend?

A) Increase in electronegativity

B) Decrease in atomic size

C) Increase in ionization energy

D) Increase in atomic size and easier electron loss

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