Periodic table - yr 10 chem

1. How are elements arranged in the periodic table?

- Increasing atomic number

2. What are the rows referred to as in the periodic table?

- Periods

3. What are the columns referred to as in the periodic table?

- Groups

4. What information does the atomic number provide about an element?

- Number of protons in the nucleus

5. What information does the mass number provide about an element?

- Number of protons and neutrons in the nucleus

6. Name the elements which has the following numbers of particles:

a. 26 electrons, 29 neutrons, 26 protons

- Iron

b. 23 protons

- Vanadium

c. 0 neutrons

- Hydrogen

7. Complete the following table;

	Electron	Neutron	Proton
Charge	Negative	No charge	Positive
Location in the atom	Outside the nucleus	Inside the nucleus	Inside the nucleus
~ Size	1/1800	1	1

8. If you know only the following information, can you always determine what the element is? (YES / NO)

a. Number of protons

- YES

b. Number of neutrons

- NO

c. Number of electrons in a neutral atom

- YES

d. Number of electrons

- NO

9. Name the following elements:

a. Group 2, period 3

- Magnesium

b. Group 17, period 4

- Bromine

c. Group 14, period 2

- Carbon

10. Complete the following table using the periodic table:

Element	Symbol	Atomic Number	Mass Number	No. of Protons	No. of Electrons	No. of Neutrons	Electron Configuration
Fluorine	19 F 9	9	19	9	9	10	2, 7
Silicon	₁₄²⁸Si	14	28	14	14	14	2, 8, 4
Mercury	120 Hg 80	80	200	80	80	120

11. Using the periodic table:

a. What are group 1 elements referred to as?

- Alkali metals

b. What are group 2 elements referred to as?

- Alkali earth metals

c. What are group 17 elements referred to as?

- Halogens

d. What are group 18 elements referred to as?

- Noble gases

e. What elements can be found in the d block?

- Transition metals

12. List 2 properties of the elements in group 8.

- Unreactive

- Gas

13. Draw electron shell diagrams for:

a. Nitrogen

b. Aluminium

14. Write the electron configuration for:

a. Carbon

- 2, 4

b. Potassium

- 2, 8, 8, 1

c. Phosphorus

- 2, 8, 5

15. How many electrons can the following shells hold: 1^st shell, 2^nd shell, 3^rd shell and 4^th shell?

1^st = 2 electrons

2^nd = 8 electrons

3^rd = 18 electrons

4^th = 32 electrons

16. What is the rule for the number of electrons each shell can hold?

- 2n²

17. Name the elements with the following electron configurations:

a. 2, 5

- Nitrogen

b. 2, 8, 8

- Argon

18. If an element has 2 electrons in its outer shell, is it a metal or non-metal?

- Metal

19. If an element has 6 electrons in its outer shell, is it a metal or non-metal?

- Non-metal

20. What is the valency of an element?

- Number of electrons in the outer shell of the atom

21. How can you use the periodic table to determine the valency of an element?

- The group number (I, II, III, IV, V, VI, VII, VIII or 1, 2, 3, 14, 15, 16, 17, 18) refers to the valency of an element (number of electrons in the outer shell)

22. Write the valency of the following elements, by using the periodic table.

a. Magnesium

- 2

b. Chlorine

- 7

c. Oxygen

- 6

23. Complete the following table, by indicating the maximum number of electrons each subshell can hold.

Subshell	Maximum number of electrons
s	2
p	6
d	10
f	14

24. Write the subshell electron configurations for;

a. Beryllium

- 1s² 2s²

b. Neon

- 1s² 2s² 2p⁶

c. Silicon

- 1s² 2s² 2p⁶ 3s² 3p²

d. Scandium

- 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹ 4s²

e. Nickel

- 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁸ 4s²

25. Compare the reactivity of group I and group II metals.

- Group I metals are more reactive than group II metals, as it is easier to remove one electron from the valence shell than 2 electrons.

26. Describe the reactivity of metals in group I and II as you go down the group.

- The reactivity increases as you move group I metals, as there are more shells so the electrons are less strongly attracted to the nucleus, therefore the 1 outer shell electron is more easily removed.

27. Explain why group 18 is referred to as noble gases.

- atoms have a full valence (outer) shell, therefore so not require to loss or gain any electrons.

28. Explain why helium is placed in group 18 and not 2.

- Helium only has 1 shell which is full, therefore it is unreactive and is a gas.

29. Describe the metallic character of the elements as you move across the period from left to right.

- Metallic character decreases, as move across the period from left to right metal to metalloids and then to non-metals.

30. State the characteristic of the oxide by a;

a. Metal

- Basic

b. Non-metal

- Acidic

· Additional Questions

1. Identify the set that contains two metals and a non-metal.

(a) Tungsten, niobium, bromine

(b) Platinum, boron, neon

(d) Tin, sodium chloride, iodine

2. Select the correct statement.

(a) There are two elements in period 2 of the periodic table.

(b)The elements of group 2 of the periodic table have two outer shell electrons.

(d) Lithium is a member of group 2.

3. Select the statement that is true of arsenic.

(a) Arsenic is a non-metal.

(b) Arsenic is a member of group 4 on the periodic table.

(d)Arsenic is a metalloid.

4. Chlorine and bromine are halogens. Which statement is true?

(a) Bromine is a red-brown liquid and chlorine is a yellow-green gas.

(b)Both are members of group 7 on the periodic table.

(d) Chlorine is a non-metal and bromine is a metalloid.

5. Decide whether each of the following statements is true or false.

(a) Calcium is an alkaline earth metal. TRUE

(b) There are 18 groups in the periodic table. TRUE

(d) All members of group 1 of the periodic table have one valence electron. TRUE

(e) All members of group 18 of the periodic table have eight valence electrons. TRUE

(f) The modern periodic table is arranged according to atomic number. TRUE

(g) The electron configuration of neon is 2,8. TRUE

(h) Silver is more reactive than mercury. FALSE

6. Complete the following table by placing the symbols of the following elements in the correct columns.

Gold	Molybdenum	Tellurium	Potassium	Silicon
Germanium	Strontium	Lead	Iodine	Radon

Metals

Metalloids

Non-metals

lead

Gold

Strontium

Molybdenum

Potassium

Silicon

Tellurium

Germanium

Iodine

Radon

7. The following table provides the atomic radius of elements in period 3 of the periodic table.

Z	11	12	13	14	15	16	17	18
Atomic radius	186	160	143	116	110	102	99	71

(a) Explain the trend in atomic radius across period 3 of the periodic table.

- As you move across period 3 in the periodic table, the atomic radius decreases

8. Two metals are chosen from a selection of metals and added to water. Metal A reacts vigorously and produces large amounts of hydrogen gas in a violent reaction. Metal B appears to have no reaction at all and simply sinks to the bottom of the water bath. What can you conclude about which metal belongs to Group I? Why do these metals behave so violently in water?

- Metal A belongs to group I. They behave so violently in water as they only have 1 electron in its valence shell, therefore it is easier for the metal to lose this 1 electron.