Download SCH3U Unit 1 review

SCH3U Unit 1 Review
List of topics covered during unit
Chemistry
Matter
Properties of matter
Physical and chemical change
Classifying matter
Atoms
Modern atomic theory
Structure of an atom
Determining protons, neutrons, electrons
Isotopes
How to calculate average atomic mass and isotopic abundance
Periodic table
Categorizing groups, periodic/group patterns 
Lewis Dot structures
Atomic size, ionization energy, electron affinity, and electronegativity trends
Ionic and covalent compounds
Predicting bonding type using electronegativity scale
Physical properties and reasoning why (intermolecular forces and intramolecular forces)
Ionic and covalent Lewis dot Structures
Diatomic atoms
Polar and non-polar bonds and molecules
Intermolecular forces
Valence shell electron repulsion theory
Geometrical and molecular shape
Review questions
1. Name the element; provide the total number of neutrons, electrons and protons from the atomic
symbol below.
Symbol
Name
Protons
Neutrons
Electrons
Hg
Iodine
47
87
2. Define the following properties as either; Qualitative physical, Quantitative physical, or Chemical.
Color
___________________________
Reactivity with acid
___________________________
Density
___________________________
Toxicity
___________________________
Physical State
___________________________
Reactivity with air
___________________________
Hardness
___________________________
Odor
___________________________
3. Explain the difference between a polar and non-polar bond. Use the following molecules to
illustrate the difference.
H - Cl
H- H
4. Identify the following bonds as Ionic, Polar covalent, or covalent. If polar, illustrate the direction of
the dipole using the vector symbol.
a. Ti---Cl
b. Na---Br
c. O---O
d. H---F
e. Cu---Se
5. The difference between an ionic bond and a covalent bond is that the cation in an ionic bond
_____________ its electrons to the anion and in a covalent bond, the electrons are _____________.
6. Determine and explain why the following processes are either a physical or chemical change.
(a) A rose bush grows from a seed that you planted and nourished.
(b) A green coating forms on a copper statue when the statue is exposed to air.
(c) Your sweat evaporates to help balance your body temperature.
(d) Frost forms on the inside of a freezer.
(e) Juice crystals dissolve in water.
(f) An ice-cream cone melts on a hot day.
7. For the following compounds, draw the Lewis Dot structure; determine the geometrical shape,
molecular shape, and polarity.
K2O
N2
AsBr3
CCl3F
SrI2
CCl4
HNC
S2
MgBr2
F2
8. Using only their locations in the periodic table, rank the atoms in each set by decreasing atomic
size.
(a) Mg, Be, Ba
(b) Ca, Se, Ga
(c) Br, Rb, Kr
(d) Se, Br, Ca
(e) Ba, Sr, Cs
(f) Se, Br, Cl
(g) Mg, Ca, Li
(h) Sr, Ca, Li
(i) In, Br, I
(j) S, Se, O
9. Using their locations on the periodic table, rank the atoms in each set by increasing
electronegativity.
(a) Sn, In, Sb
(b) Sr, Ca, Ba
(c) K, Ca, Rb
(d) C, Br, F
10. Explain why ionic compounds generally have a higher melting point when compared to covalent
compounds.
12. What is hydrogen bonding, and why does this intermolecular force cause water molecules to be
attracted to each other?
13. What are London Dispersion forces? Why are they so weak?
14. In nature, silicon is composed of three isotopes. Calculate the average atomic mass of silicon for
the values below.
27.98 u 92.23%
28.97 u 4.67%
29.97 u 3.10 %
15. Lead occurs naturally as fur isotopes. Calculate the average atomic mass of lead from the values
below.
204.0 u
206.0 u
207.0 u
208.0 u
1.37%
26.26%
20.82%
51.55%
16. Naturally occurring silver exists in two isotopes, and has an average atomic mass of 107.9 u. From
the values below, calculate the isotopic mass of silvers second isotope (solve for X below).
Isotope 1: 106.9 u 51.8 %
Isotope 2: X
48.2 %