Download Science 10 Chemisry Quiz

Science 10 Quiz
Name- ____________________________________________
This test is open book, so use your notes, but it is not a group activity
1) Fill in the following chart (12 marks)
Symbol
# protons
# electrons
# neutrons
Charge
Na
Cl26
35
32
36
+3
45
2) In the space below, draw a representation of the Lithium atom (3 marks)
3) Draw a representation of the Magnesium ion (3 marks)
4) Fill out the following table (3 marks)
Symbol
Name
CaCl2
K2O
BeI2
5) Fill out the following table (4 marks)
Name
Symbol
Calcium Phosphide
Potassium Bromide
Strontium Nitride
Barium Oxide
6. Chemical substances written to the right of the arrow in an equation are called
a) products
b) reactants
c) subscripts
d) coefficients
7. Which set of coefficients correctly balances the following reaction?
__ S8(s) + __ P4(s)  __ P4S3(s)
a)
b)
c)
d)
8, 3, 8
3, 8, 8
6, 8, 4
1, 1, 1
8. What is the missing coefficient in the equation?
C3H8(g) + ? O2(g)  3 CO2(g) + 4H2O(g)
a)
b)
c)
d)
2
5
6
10
9. What is the mass of 2.00 moles of silver?
a) 2.00 g
b) 109 g
c) 216 g
d) 6.02 x 1023 g
Balance each equation
10. ____ AlCl3(s)  ____ Al(s) + ____ Cl2(g)
11. ____ Mg(s) + ____ H3PO4(aq)  ____ H2(g) + ____ Mg3(PO4)2(s)
12. ____ Na2CO3(aq) + ___ H3PO4(aq)  ___ Na3PO4(aq) + ___ H2O(l) + ___ CO2(g)
13. How many moles of water are in 72.08 g of H2O(l)? (1 mark)
14. The periodic table organizes all the elements according to
a) date of discovery
b) physical properties
c) chemical properties
d) chemical importance
15. Which of the following pieces of information is not shown on the periodic table?
a) the mass number
b) the element name
c) the atomic number
d) the element symbol
16. Which of the following applies to metallic elements when they form positive ions?
a) they lose electrons and become anions
b) they lose electrons and become cations
c) they gain electrons and become anions
d) they gain electrons and become cations
17. Sometimes when ionic solutions are mixed, they form a precipitate. A precipitate is
a) an electrolyte
b) a mixture of dissolved ions
c) a solid substance that forms when two liquids are mixed
d) an aqueous substance that forms when two liquids are mixed
Write the formula or name of the compounds in questions 11 to 16. (6 marks)
18. sodium sulfide
19. iron(III) nitrate
20. dinitrogen trioxide
21. Al2N3(s)
22. P4O10(s)
23. (NH4)2CrO4(s)
24. Which column in the periodic table contains elements with one electron in their
valence energy level?
a) first on the left
b) first on the right
c) second from the left
d) second from the right
25. Which two particles are approximately equal in mass?
a) proton and neutron
b) proton and electron
c) neutron and electron
d) none of these
26. The magnesium ion, Mg+2, has
a) 10 electrons and 10 protons
b) 10 electrons and 12 protons
c) 12 electrons and 10 protons
d) 12 electrons and 12 protons
27. An atom of fluorine has 9 protons, 10 neutrons, and 9 electrons. Its mass number is
a) 9
b) 10
c) 18
d) 19
28. What is the formula for sodium carbonate?
a) S2CO3(s)
b) NaCO(s)
c) Na2CO3(s)
d) Na3CO3(s)
29. What is the formula for aluminium hydroxide?
a) AlOH3(s)
b) Al3OH(s)
c) Al(OH)3(s)
d) Al(III) OH(s)
30. Which of the following is an ionic compound?
a) HCl(g)
b) KCl(s)
c) ClO3(g)
d) NCl3(g)
31. Consider the following reaction:
____ NaOH(aq) + ____ Al(NO3)3(aq)  ____ Al(OH)3(s) + ____ NaNO3(aq)
The coefficient for Al(NO3)3 when the above equation is balanced is
a) 1
b) 2
c) 3
d) 4
32. The molar mass of chlorine gas is:
a) 35.45 g/mol
b) 70.90 g/mol
c) 141.8 g/mol
d) 283.6 g/mol
33. What is the mass of 3.00 mol of calcium?
a) 3.00 g
b) 9.00 g
c) 40.1 g
d) 120 g
34. What is the mass of 1.00 mole of H2O(l)? (1 mark)
35. What is the mass of 4.00 moles of Fe? (2 marks)
36. How many moles of carbon dioxide are in 440.1 g of CO2(g)? (2 marks)
Name or give the formula for each compound
37.
CaBr2(s)
38.
Au3PO4(s)
39.
N2O4(g)
40.
NH3(s)
41.
H2SO4(aq)
42.
lead(IV) sulfide
43.
methane
44.
sulfur trioxide
45.
hydrochloric acid
46.
iron(II) nitride
Balance the equations in questions
47. _____ Na(s) + _____ O2(g)  _____ Na2O(s)
48. ______ C8H16(l) + ______ O2(g)  ______ CO2(g) + ______ H2O(g)
49. ______ NH3(g) + _____ O2(g)  ______ NO(g) + _____ H2O(l)
Write balanced formula equations for the reactions
50. Aqueous ammonium sulfide and aqueous lead(II) nitrate are mixed together. They
react to yield aqueous ammonium nitrate and solid lead(II) sulfide. (2 marks)
51. Copper metal is placed in a solution of silver nitrate. This produces aqueous
copper(II) nitrate and silver metal. (2 marks)
52. The element nitrogen has two common isotopes: nitrogen-14 and nitrogen-16.
a) State how these two types of atoms are similar. (1 mark)
b) State how these two types of atoms are different. (1 mark)