Download The Periodic table and subatomic particles

SCH3U
Grade 9 and 10 Chemistry Review
Date: ________________________
The Periodic table and subatomic particles
In the periodic table, for each element:
Remember the following relationships:
Atomic Number = the # of protons = the # of electrons (in a neutral atom)
Mass Number = the atomic mass of the most common isotope (round the average atomic mass to the nearest whole
number)
Ex. For cobalt: Average Atomic Mass = 58.93 ≈ 59 = Mass Number
Atomic Notation
Number of Neutrons = Mass Number – Number of Protons
Ex. For cobalt: Number of neutrons = 59 – 27 = 32 neutrons
1. Complete the following chart:
Element
Atomic
Symbol
Name
notation
11
5
Atomic
number
Mass
number
# of
protons
# of
neutrons
B
Silver
82
14
# of
electrons
Bohr-Rutherford Diagrams
 Diagram showing arrangement of subatomic particles in an atom.
 Electron arrangement for first 20 elements is 2, 8, 8, 2.
 Arrangement within the atom is reflected in the row and period number on the
periodic table.
o Row # = number of orbitals (energy levels)
o Period # number of valence electrons.
2. Draw Bohr-Rutherford Diagrams for the following:
a) magnesium atom
b) the noble gas in the 3rd row
c) sodium ion
d) fluorine ion
Counting atoms:
Coefficients  apply to all atoms in the compound.
Subscripts  apply only to the element that they follow.
Exception – if the subscript follows a bracket “)”, it is applied to all elements in the bracket.
Ex. For calcium nitrate 2Ca(NO3)2




The coefficient (2) applies to all elements:
Therefore: 2 Ca atoms total
2 N atoms (not total)
The subscript 3 only follows O so we have 2 x 3 O = 6 O
The subscript 2 is outside brackets, so it applies to N and O
o Therefore, 2 x 6 O = 12 oxygen atoms total
o 2 x 2 N = 4 nitrogen atoms total
2 O atoms (not total)
3. Give the name of each element and state the number of atoms of each element in the following compounds:
CH3COOH
Name of element
2(NH4)2Cr2O7
# of atoms
Name of element
# of atoms
Chemical Reactions
Chemical reactions produce NEW substances by the
breaking and forming of BONDS.
4. The four indicators that a new substance has
formed (chemical change).
1. Change of________________
2. Formation of a ________________
3. Formation of _____________
4. Release or absorption of_____________
Names and Formulas:



Ionic compounds – metal and nonmetal – name metal and change ending of nonmetal to “ide”
Molecular compounds – 2 nonmetals (use prefixes)
Polyatomic compounds – metal and group of nonmetals – name metal followed by polyatomic ion
5. Complete the following table:
Chemical Name
magnesium hydroxide
Ions present (use
“NA” if not present)
Mg2+
Chemical Formula
OH-
Mg(OH)2
Ni(NO3)2
beryllium iodide
N2O5
lead(II) nitrite
fluorine gas
aluminum sulfate
silicon dioxide
Balancing Chemical Equations:
Add coefficients to each chemical formula (if needed), so that the same numbers of atoms of each element are
found on both sides of the arrow.
Not sure where to start?? Try using the “MINOH” method, by balancing elements in the following order:
M – metals
I – polyatomic ions
N – non-metals
O – oxygen
H – hydrogen
6. Balance the following equations:
____ AlBr3 + ____ K  ____ KBr + ____ Al
____ P4 + ____ Br2  ____ PBr3
____ CoBr3 + ____ CaSO4  ____ CaBr2 + ____ Co2(SO4)3
____ Na3P + ____ CaF2  ____ NaF + ____ Ca3P2
____ Mn + ____ HI  ____ H2 + ____ MnI3
7. Why do we need to balance chemical equations?
8. A 10th grade science class is studying the law of conservation of mass.
Reactants, magnesium and hydrochloric acid are massed before and after
their reaction in an open Erlenmeyer flask. The following data is obtained:
Substance
Hydrochloric acid
and flask
Magnesium ribbon
Flask and
products
Mass
150.3 g
a. Write and word and chemical equation for the reaction.
b. Does this defy the law of conservation of mass? Explain.
Predicting products of reactions and reaction types:





Synthesis – 2 simpler reactants form more complicated product
Decomposition – Reactant breaks down into more than 1 product
Single displacement – metal and ionic compound
Double displacement – 2 ionic compounds
Combustion – hydrocarbon reacts with oxygen to form water and
carbon dioxide
8. Complete the following table:
Balance and predict products
a) __BaO2 __BaO + __O2
b) __C6H6 + __O2

c) __H2 + __O2 
d) __K + __Ca(NO3)2 
e) __CaCl2 + __Na2CO3 
Type of reaction
1.1 g
149.8 g
Acids and Bases



pH scale – measures acidity, each 1 unit change is a 10 fold change in level of acidity (H+ concentration)
acid – substance that ionizes to release hydrogen ions (HCl)
base – substance that dissociates to release hydroxide ions (NaOH)
9. Indicate whether the following characteristics refer to acids or bases by putting a check mark ( ) in the
appropriate box.
Characteristic
Acids
Bases
Both
Good conductors of electricity (electrolytes)
React with carbonates to produce CO2(g)
Will cause blue litmus paper to change red
Will cause red litmus paper to change blue
Sour taste (*NOTE: do not taste or touch in the lab)
Have a pH greater than 7
Taste bitter and feel slippery (*NOTE: do not taste
or touch in the lab)
Have a pH less than 7
React with active metals to produce H2(g)
REVIEW ASSESSMENT
To prepare for your test you should:
1. Read over notes in this package.
2. Redo these worksheets as well as extra practice sheets that have been provided.
3. Go through your grade 9 and 10 notes (should you still have them).
4. Topics to be covered include:
Periodic table and its organization, subatomic particles, Bohr-Rutherford diagrams, ions, counting atoms,
chemical reactions, names an formulas, balancing chemical equations, law of conservation of mass, reaction types,
words and chemical equations, acids and bases, process of scientific inquiry, safety and reading MSDS sheets.
REVIEW TEST DATE: _________________________________
Balancing Worksheet #1
Please note that several of these equations are already balanced as written.
1.
H2 +
O2 --->
H2O
2.
S8 +
O2 --->
SO3
Answers:
3.
HgO --->
Hg
O2
4.
Zn +
HCl --->
ZnCl2 +
H2
5.
Na +
H2O --->
NaOH +
H2
6.
C10H16 +
Cl2 --->
C+
HCl
7.
Si2H3 +
O2 --->
SiO2 +
H2O
8.
Fe +
O2 --->
Fe2O3
9.
C7H6O2 +
O2 --->
CO2 +
H2O
10.
FeS2 +
O2 --->
Fe2O3 +
SO2
11.
Fe2O3 +
H2 --->
Fe +
H2O
12.
K +
Br2 --->
KBr
13.
C2H2 +
O2 --->
CO2 +
14.
H2O2 --->
H2O +
O2
1. 2, 1 ---> 2
2. 1, 12 ---> 8
3. 2 ---> 2, 1
4. 1, 2 ---> 1, 1
5. 2, 2 ---> 2, 1
6. 1, 8 ---> 10, 16
7. 4, 11 ---> 8, 6
8. 4, 3 ---> 2
9. 2, 15 ---> 14, 6
10. 4, 11 ---> 2, 8
11. 1, 3 ---> 2, 3
12. 2, 1 ---> 2
13. 2, 5 ---> 4, 2
14. 2 ---> 2, 1
15. 1, 11 ---> 7, 8
16. 1, 4 ---> 1, 2
17. 2 ---> 2, 3
18. 4 ---> 3, 1
19. 1, 6 ---> 4
20. 4, 3 ---> 1
21. 1, 5 ---> 3, 4
22. 1, 3 ---> 2, 3
23. 1, 4 ---> 5, 1
24. 8, 8 ---> 1, 16
25. 3, 4 ---> 1, 4
15.
C7H16 +
O2 --->
CO2
+
H2O
16.
SiO2 +
HF --->
SiF4
+
H2O
17.
KClO3 --->
KCl
O2
18.
KClO3 --->
KClO4 +
KCl
19.
P4O10
H2O --->
H3PO4
20.
Sb +
O2 --->
Sb4O6
21.
C3H8 +
O2 --->
CO2
+
H2O
22.
Fe2O3 +
CO --->
Fe +
CO2
23.
PCl5
H2O --->
HCl +
H3PO4
24.
H2S +
Cl2 --->
S8 +
HCl
25.
Fe +
H2O ---> Fe3O4
+
+
+
+
+
H2O
H2