Ions quiz

1. What is needed to complete this diagram to show the ionic bonding in potassium oxide, K₂O ?

1) eight electrons around the oxide (six dots and two cross) 2) A charge of +1 on the potassium and -2 on the oxide 3) A second oxide ion the same as the first

1) eight electrons around the oxide (six dots and two cross) 2) A charge of +2 on the potassium and -1 on the oxide 3) A second potassium ion the same as the first

1) eight electrons around the oxide (six dots and two cross) 2) A charge of +1 on the potassium and -2 on the oxide 3) A second potassium ion the same as the first

1) eight electrons around the potassium (any combination of dots and one crosses) 2) A charge of +2 on the oxide and -1 on the potassium 3) A second potassium ion the same as the first

Question 1 of 22

2. If copper chloride has the formula CuCl₂, what is the formula of the copper ion?

Cu⁺

Cu²⁺

Cu²⁻

Cu⁻

Question 2 of 22

3. State the electron configuration of the sulfide ion

8,8,2

2,8,8

2,8,2

2,8,8,2

Question 3 of 22

4. How many electrons in a helium atom?

1

2

3

4

Question 4 of 22

5. How many electrons can the first, second and third shells hold?

First 8, second 8, third 8

First 2, second 6, third 6

First 0, second 8, third 8

First 2, second 8, third 8

Question 5 of 22

6. Why do ionic substance have high melting and boiling points?

There are weak intermolecular forces, in a simple molecular structure, which require little energy to overcome

There is a weak electrostatic attraction between oppositely charged ions, in a giant structure, which requires little energy to overcome

There is a strong electrostatic attraction between similarly charged ions, in a giant structure, which requires a lot of energy to overcome

There is a strong electrostatic attraction between oppositely charged ions, in a giant structure, which requires a lot of energy to overcome

Question 6 of 22

7. On the Periodic table what is the meaning of the word Group? What does that tell us about the electron configuration of the atom?

Same number of electron shells

Same number of electrons in the inner shell

Same electronic configuration

same number of electrons in the outer shell

Question 7 of 22

8. Which group of atoms has a full outer shell?

Group 0, the noble gases

Group 1, the alkali metals

Group 2, alkaline earth metals

Group 7, the halogens

Question 8 of 22

9. On the Periodic Table what is the meaning of the word Period? What does that tell us about the electron configuration of the atom?

same number of electron shells

same number of electrons in the outer shell

Same number of electrons in the inner shell

Same electronic configuration

Question 9 of 22

10. State the formula of the hydrogen ion

H⁻

H₃O⁺

H⁺

H₃O⁻

Question 10 of 22

11. State the electron configuration of the oxide ion

8,2

8,8

2,8

2,6

Question 11 of 22

12. What is the formula for iron (II) phosphide?

Fe₂P

FeP₂

Fe₃P₂

Fe₂P₃

Question 12 of 22

13. Balance the following equation: WO₃ + H₂ → W + H₂O

2WO₃ + 3H₂ → 2W + 6H₂O

WO₃ + 6H₂ → W + 3H₂O

WO₃ + 3H₂ → W + 6H₂O

WO₃ + 3H₂ → W + 3H₂O

Question 13 of 22

14. Explain, in terms of structure and bonding, why sodium chloride has a very high melting point

NaCl has a simple molecular structure with weak intermolecular forces that require little energy to break

NaCl has a giant ionic structure with strong electrostatic forces between oppositely charged ions that require a lot of energy to break

NaCl has a simple molecular structure with strong electrostatic forces between oppositely charged ions that require a lot of energy to break

NaCl has a giant ionic structure with weak electrostatic forces between oppositely charged ions that require little energy to break

Question 14 of 22

15. How can atoms get a full outer shell?

Either the transfer (covalent) or sharing (ionic) of electrons

Either the transfer (ionic) or sharing (covalent) of electrons

Conversion of electrons to protons

Only transfer (ionic) of electrons

Question 15 of 22

16. Explain, in terms of electrons, why isotopes have the same chemical properties

Isotopes have the same number of protons but a different number of neutrons

Isotopes have the same number of electrons

Isotopes have different masses

Isotopes are radioactive

Question 16 of 22

17. When are ions attracted to each other?

When the ions are the same size

When the ions are very small

When the ions are oppositely charged

When the ions have the same charge

Question 17 of 22

18. What holds ions together?

Ions are held together by a strong electrostatic attraction between the shared pair of electrons and their nuclei

Ions are held together by a strong electrostatic attraction between the oppositely charged ions

Ions are held together by a strong magnetic attraction between the oppositely charged ions

Ions are held together by a strong electrostatic attraction between the similarly charged ions

Question 18 of 22

19. Balance the equation for the reaction: ___ HCl(aq) + ___ MnO₂(s) → ___MnCl₂(aq) + ___H₂O(l) + ___ Cl₂(g)

4 HCl(aq) + 2 MnO₂(s) → 2 MnCl₂(aq) + 2H₂O(l) + Cl₂(g)

4 HCl(aq) + MnO₂(s) → MnCl₂(aq) + 2H₂O(l) + Cl₂(g)

6 HCl(aq) + MnO₂(s) → MnCl₂(aq) + 2H₂O(l) + 2 Cl₂(g)

2 HCl(aq) + MnO₂(s) → MnCl₂(aq) + H₂O(l) + Cl₂(g)

Question 19 of 22

20. What are the elements in group 0 called?

Light gases

Halogens

Noble gases

Alkali metals

Question 20 of 22

21. What is the formula for copper (II) fluoride

CuF

CuF₂

Cu₂F₂

Cu₂F

Question 21 of 22

22. Why do elements in the same group of the periodic table have similar chemical properties?

Elements in the same group of the periodic table have different numbers of electrons in their outer shell

Elements in the same group of the periodic table have the same number of electrons in their outer shell

Elements in the same group of the periodic table are all the same type of element (metal, non-metal etc.)

Elements in the same group of the periodic table have the same number of protons

Question 22 of 22

Ions quiz

Ions quiz

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