Download Year 11 Chemistry Balancing Equations

Year 11 Chemistry
Balancing Equations
1.
____ Sb + ____ Cl2  ____SbCl3
2.
____ Mg + ____O2  ____MgO
3.
____ CaCl2  ____ Ca + ____ Cl2
4.
____ NaClO3  ____ NaCl + ____ O2
5.
____ Fe + ____ HCl  ____ FeCl2 + ____ H2
6.
____ CuO + ____ H2  ____ Cu + ____ H2O
7.
____ Al + ____ H2SO4  ____ Al2(SO4)3 + ____ H2
8.
____ MgBr2 + ____ Cl2  ____ MgCl2 + ____ Br2
9.
____ SnO2 + ____ C  ____ Sn + ____ CO
10.
____ Pb(NO3)2 + ____ H2S  ____ PbS + ____ HNO3
11.
____ HgO  ____ Hg + ____ O2
12.
____ KClO3  ____ KCl + ____ O2
13.
____ N2 + ____ H2  ____ NH3
14.
____ NaBr + ____ Cl2  ____ NaCl + ____ Br2
15.
____ Zn + ____ AgNO3  ____ Zn(NO3)2 + ____ Ag
16.
____ Sn + ____ Cl2  ____ SnCl4
17.
____ Ba(OH)2  ____ BaO + ____ H2O
18.
____ Mg(OH)2 + ____ HCl  ____ MgCl2 + ____ H2O
19.
____ Na2CO3 + ____ HCl  ____ NaCl + ____ H2CO3
20.
____ NH4NO2  ____ N2 + ____ H2O
21.
____ N2 + ____ O2  ____ N2O5
22.
____ MgCO3  ____ MgO + ____ CO2
23.
____ KBr + ____ Cl2  ____ KCl + ____ Br2
24.
____ Zn + ____ CuSO4  ____ Cu + ____ ZnSO4
25.
____ P + ____ O2  ____ P4O6
26.
____ SrBr2 + ____ (NH4)2CO3  ____ SrCO3 + ____ NH4Br
27.
____ AgNO3 + ____ (NH4)2CrO4  ____ Ag2CrO4 + ____ NH4NO3
28.
____ K + ____ H2O  ____ KOH + ____ H2
29.
____ Al + ____ Pb(NO3)2  ____ Al(NO3)3 + ____ Pb
30.
____ Fe + ____ O2  ____ Fe3O4
_
1
Mass
Number
Chemistry: Atomic Number and Mass Number
23 Na
11
Complete the following chart and answer the questions below.
Element
Name
Atomic
Number
Number of
Protons
Symbol
for
Sodium
Atomic Number
11 Protons
Number of
Neutrons
carbon
Mass Number
12
8
8
hydrogen
1
6
hydrogen
14
2
nitrogen
14
1
92
2
146
cesium
82
11
12
47
tungsten
108
110
45
24
80
52
89
silver
152
107
76
114
How are the atomic number and the number of protons related to each other?
How do the number of protons, number of neutrons, and the mass number relate to each other?
What is the one thing that determines the identity of an atom (that is, whether it is an oxygen atom or a carbon atom,
etc.)?
2
Complete the following questions
1.
Isotope
12
6
C
Element
Atomic
Number
Mass
Number
Carbon
6
12
Number of
Neutrons
Number of
Electrons
Electron Shell
Configuration
6
2, 4
2, 4
13
6
C
14
6
C
12
23
H
1
Ca
20
1
1
40
20
27
13
Al
Argon
Silicon
Iodine
20
30
127
74
2.
If an element has two electrons in its outer shell, is it a metal or non-metal? Explain your answer
__________________________________________________________________________________
__________________________________________________________________________________
___________________________________________________________________________________
3.
What is special about elements that have eight electrons in their outer shell?
___________________________________________________________________________________
________________________________________________________________________________
4. How many shells are filled or partly-filled for a Period 3 element?
______________________________________________________________
5. State the number of outer shell electrons for elements in:
a. Group 1 ________
b. Group 3 ________
c. Group 7 ________
d. Group 5 ________
6.
How many electrons do the following have?
a.
An atom with 6 protons ________
b. An atom with atomic number 17________
c.
d. An atom with Period 3, Group V ________
e. A sulfur atom ________
An atom in Period 2, Group III ________
3
7. Draw the electronic arrangement for the following elements
a. oxygen
b. sodium
c. sulfur
8.
d. potassium
What is the difference between an element and a compound?
9.
Explain the following terms:
A
isotopes
B
mass number
C
subshell
D
valence electron
E
orbital
F
ground state
10.
Compare the mass and charge of protons, electrons and neutrons.
11.
What is the maximum number of electrons in the second shell?___________________
4
12.
13.
Discuss the contributions made to our understanding of the atom by the following scientists:
A
John Dalton
B
J J Thompson
C
James Chadwick
D
Ernest Rutherford
E
Niels Bohr
F
Erwin Schrodinger
(write your answers in your chemistry module)
Write out the electron configuration for each of the following elements.
1. H
2. Li
3. Na
4. K
5. Rb
6. Be
7. Mg
8. Ca
9. Sr
10. C
11. O
12. S
13. F
14. Cl
15. Br
16. I
17. He
18. Ne
19. Ar
20. Kr
21. Xe
22. F
Looking over your electron configurations, are there any elements above that have similar valence electron
configurations to those of other elements? If so, list below the elements that are similar (in terms of valence
electrons) and state the similarity for each of the groups.
5
14. Give the chemical symbol for any element:
a
in the same group as fluorine (F) _______________
b
in the same period as sodium (Na) ________________
c
in the group known as the alkali metals _____________
d
that would form ions of charge 3 _________________
15.
List three properties of non-metals
16.
List three properties of metals.
17. Listed below are five atoms using symbols that are not the usual symbols of the elements. Use the letters V
to Z to answer the following questions.
40
18 V
20
10 W
40
19 X
39
19 Y
40
20 Z
a
Which two atoms have the same number of neutrons?
________________
b
Which atom has the smallest mass number? ____________________
c
 thesameelement?
 _____________________
Which two atoms belong to
d
Which two symbols represent noble gases? _______________________
18. State one way in which helium (He) is:
a
like all other gases in Group VIII
b
different from all other gases in Group VIII
19.
Write balanced chemical equations, including subscripts, for each of the following reactions.
Follow these steps:
• Write the word equation for the reaction.
• Directly underneath the word equation, write the unbalanced formula equation.
• Add subscripts—(s), (l), (g) or (aq).
• Balance the equation. (don’t change any FORMULA e.g. CO2 does not change when you
balance the equation but you may have 2CO2 or 3CO2 etc.)
Note: ‘Dilute’ means a water solution, and therefore the appropriate subscript is (aq)
Write these equations in your moodule
a. Dilute hydrochloric acid HCl is added to solid magnesium hydroxide Mg(OH)2, producing water and the
soluble salt magnesium chloride MgCl2.
b. Dilute nitric acid HNO3 is added to solid calcium carbonate CaCO3, producing bubbles of carbon dioxide,
water, and the soluble salt calcium nitrate Ca(NO3)2
c When dilute sodium sulfate Na2SO4 solution is added to dilute barium nitrate Ba(NO3)2 solution, barium
sulfate BaSO4 precipitates, leaving sodium nitrate NaNO3 in solution.
d Dilute sodium hydroxide is added to dilute sulfuric acid H2SO4, producing water and the soluble salt sodium
sulfate Na2SO4
e Dilute sulfuric acid is poured over solid sodium carbonate Na2CO3, producing carbon dioxide, water and the
soluble salt sodium sulfate.
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7
8