C2.2 Chemical Families – LearnITbyTests

1. Mention the physical properties of Halogens

Fluorine and chlorine are gaseous at room temperature while bromine is brown liquid and iodine a shiny dark grey solid

The solubility of halogens in water decreases down the group

Halogens are non-conductors of heat and electricity

All of the above

2. Mention the chemical properties of alkali metals

Alkali metals react with water to form alkaline solutions and hydrogen gas

Alkali metals react with chlorine gas to form metal chlorides.

Alkali metals react with oxygen to form a base

Both A and B

3. Explain why there is an increase in reactivity as you go down the alkali metal group from Lithium to Potassium

Due to the ease of losing valence electrons increases down the group as the atomic radius increases

The most reactive metal which is Potassium its outermost electron is easily removed during a reaction

The atomic radius decreases as you go down the group

Both A and B

4. Due to their reactivity alkali metals are not found as free electrons rather as combined elements

FALSE

Maybe

TRUE

None

5. Which of the following statement describes the characteristics of alkaline earth metals?

It has two electrons in the outermost energy level

Its atomic radius increases as you go down the group

Its ionic radius reduces as you go down the group

All of the above

6. How many alkali metal ions is needed to combine one oxide ion?

7. Mention the physical properties of Alkali metals

Alkali metals have a shiny metallic luster when cut which quickly tarnishes as it reacts with the surrounding air.

Alkali metals are soft and easy to cut

Alkali metals have low melting and boiling points

All of the above

8. Which of the following doesn’t belong to alkaline earth metals?

Magnesum

Beryllium

Calcium

Sodium

9. Mention the examples of Halogens

Fluorine

Chlorine

Bromine

All of the above

10. What is the name of the energy released as an ion is formed in halogen?

Ionization energy

Electron affinity

Cation

Anion

11. Does the electron affinity decrease as the size of the atoms increases in Halogen hence the reactivity decreases down the group? {Fluorine reacts more than iodine} True or False

TRUE

FALSE

Maybe

None

12. Which of the following is not a noble gas?

Helium

Neon

Argon

Chlorine

13. Explain why Halogens cannot conduct heat and electricity

Absence of delocalized electrons

Presence of delocalized electrons

Absence of mobile atoms

None of the mentioned

14. The elements in group 8 of the periodic table are called

Halogens

Alkaline metals

Alkaline earth metals

Noble gases

15. In Alkali metals, the electrons in the outermost energy level move randomly throughout the metallic structure and are said to be delocalized?

TRUE

FALSE

Maybe

None

16. Does the ionization energy decrease as you go down the group of alkali metals?

FALSE

Maybe

TRUE

None

17. Mention the uses of alkali metals and their compounds

Lithium compounds are used in the manufacture of mobile phone dry cells

Sodium chloride is used as a food additive.

Molten sodium is used as a reducing agent in the extraction of titanium

All of the above

18. Mention the uses of Halogens and their compounds

Chlorine is used to make bleaches used in paper pulp.

Chlorine is added to water to kill micro-organisms

Fluorine is used to manufacture hydrogen fluoride used to engrave words or pictures

All of the above

19. Why is the atomic radius of halogen atom less than the ionic radius of halogen ion?

Halogen atom gains an electron in the outermost energy level to become an ion

Halogen atom loses an electron in the outermost energy level to become an ion

Halogen atom loses all the electron in the outermost electron to become an ion

None of the mentioned

20. Which among the following element is not among Period 3?

Sodium

Potassium

Magnessium

Aluminium

21. Mention the characteristics of Noble gases

Their outermost energy level is full with Helium (2) duplet and the rest have (8) octet

Neither gain nor lose electrons

They are stable and non-reactive

All of the above

22. Which of the following is not an example of alkali metal?

Calcium

Lithium

Sodium

Potassium

23. Mention the uses of Alkaline earth metals and their compounds

Magnesium is used in the manufacture of magnesium hydroxide which is used as anti-acid medicine.

Calcium carbonate is used in the extraction of iron.

Magnesium oxide is used in the lining of furnaces.

All of the above

24. The atomic radius of Halogen atom is less than the ionic radius of halogen ion e.g. Chlorine atom and Chlorine ion True or False

TRUE

FALSE

Maybe

None

25. Mention the uses of noble gas

Argon is used in light bulbs to provide an inert environment to prevent oxidation

Argon is used as an insulator in arch-welding

Neon gas is used in street and advertisement light

All of the above

26. The elements in group 1 of the periodic table are called Alkali metals True or False

TRUE

FALSE

Maybe

None

27. Explain why Halogen melting and boiling point level increase as you go down the group? {Iodine has high melting and boiling point than Fluorine}

Presence of delocalized electrons

Intermolecular forces increase with the increase in the size of the molecules

Force of attraction decreases with the size of the molecules

None of the mentioned

28. Mention the chemical properties of Halogens

It reacts with metals to form Metal chloride ( salt)

It reacts with water to form an acid.

Chlorine + water + Hydrochloric acid + Chloric (I) acid

All of the above

29. Explain why the melting and boiling points decrease down the group of alkali metals

Due to the weakening of the forces holding the atoms together

As the atomic radius increases as you go down the group the forces of attraction between the atoms weaken

Both A and B

None of the mentioned

30. What is the name of the minimum energy required to remove an electron from the outermost energy level of an atom in the gaseous state?

Ionic radius

Atomic radius

Ionization energy

None of the mentioned

31. Explain why are alkali metals are good conductors of heat and electricity

Presence of delocalized (free) electrons

Absence of free electrons

Presence of mobile atoms

None of the mentioned

32. Mention the characteristics of Halogens

The atomic radii increase down the group

The ionic radii increase down the group

An increase in the number of occupied energy levels.

All of the above

33. Mention the physical properties of Alkaline earth metals

When alkaline earth metal is polished it acquires a metallic luster and you must polish it before an experiment in order to remove the thin oxide layer which forms on the surface

They are good conductors of electricity and have high melting and boiling points

They are brittle (calcium) and ductile (magnesium) hence hard to cut with a knife

All of the above

34. Mention the physical properties of noble gases

Are colorless monoatomic gases

Their atomic radius increases down the group due to the increase in the number of energy levels

Have a low melting and boiling points due to weak inter-atomic forces of attraction between atoms

All of the above

35. Mention the physical properties of elements in period 3

The atomic radii decrease across the period from left to right of the periodic table

High melting and boiling points of aluminum compared to metals sodium and magnesium

The high melting point of silicon compared to non-metals Phosphorous and Chlorine

All of the above

36. The elements in Group 2 of the periodic table are called?

Alkali metals

Form two's

Alkaline earth metals

None of the mentioned

37. Explain why is the ionic radius of an alkali metal is less than its atomic radius

An alkali metal forms an ion by losing the single electron from the outermost energy level.

The resulting ion {cation} has one less occupied energy level than the alkali atom

The ionic radius is nearer to the nucleus than the atom

Both A and B

38. Mention the Electrical physical properties of elements in period 3

Some such as Sodium, Magnesium, and Aluminum conduct electricity due to the presence of delocalized electrons

Some do not conduct electricity such as Phosphorous, Sulphur, and chlorine which are molecules are lack delocalized electrons

Some like Silicon are semi-conductors

All of the above

39. Define Atomic Radius?

The distance between the center of the nucleus of an atom and the innermost energy level occupied by an electron(s

The distance between the nucleus and the outermost energy level

The distance between the center of the nucleus of an atom and the outermost energy level occupied by an electron(s).

None of the mentioned

40. Explain why the ionization energy decreases as you go down the group of alkali metals

Increase in the atomic size as you down the group

he decrease in the force of attraction between the positive nucleus and the negative outermost electron.

Increase in the atomic radius as you go down the group

All of the above

41. Explain why atomic radii of the alkali metals increase down the group

Each alkali metal has one more occupied energy level than the preceding member in the group

Alkali metals have one valence electron in the outermost energy level

Alkali metals lose an electron to form a positively charged ion

None of the mentioned.

42. Non-metals in Group 7 are called

Alkali

Alkaline earth metals

Halogens

None

43. Mention the chemical properties of Alkaline earth metals

They react in the air to form Metal oxides and react with water to form alkaline solution and hydrogen gas.

Magnesium reacts with steam to give Magnesium oxide and hydrogen gas

Alkaline earth metals react with chlorine to give out Metal chloride (Magnesium Chloride and Calcium chloride).

All of the above

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