Download SCH3U Course Review

1
Grade 11 Chemistry Mid-Term Review
Properties of Matter
1. State or explain MATTER and its three states.
2. State and explain the classification of matter.
3. Explain and illustrate your explanation of the following:
a) mechanical mixture
b) characteristic physical property
c) characteristic chemical property
d) physical change
e) chemical change (reaction)
f) qualitative observation ( property)
g) quantitative observation ( property)
h) element
i) compound
j) homogeneous mixture
k) heterogeneous mixture
l) kinetic energy
m) potential energy
4. Classify as either a PHYSICAL or a CHEMICAL property and justify.
a) density b) boiling point of pure water c) colour of carrots
d) sodium bicarbonate decomposes to carbon dioxide and sodium carbonate and
water.
5. Classify each of the following as a CHEMICAL or a PHYSICAL change and
justify:
a) darkening of silver
b) fermenting of grapes
c) formation of snow flakes
d) sculpturing of soap
6. Describe how you would separate a mixture of salt, sand, and iron filings.
7.
a)
b)
c)
d)
e)
Ionization energies tend to
increase with increasing atomic radii
decrease with increasing nuclear charge
decrease across a period from left to right
increase across a period from left to right
increase as you go down a family
8. The bond in HCl (hydrogen chloride) is said to be polar covalent because
a) hydrogen chloride molecules are relatively weakly held together
b) the shared electron pair is closer to the one atom than to the other
c) chlorine has a much higher atomic number than hydrogen
d) chemical bonds consist of electrical forces between atoms
e)the bond results from minimum potential energy
2
Structure of the Atom
1. State the following laws of chemical change:
a) Law of Conservation of Mass
b) Law of Constant Composition
2.State Dalton's Atomic Theory.
3. Explain: a) atomic mass unit, b) atomic mass, c) electron, d) proton, e) neutron,
f) isotope, g) atomic number, h) mass number, i) line spectrum, l) energy
level(orbit), m) electron arrangement
4. Outline the contribution of the following to our understanding of atomic structure.
Your discussion should focus on the evidence that supports each model proposed.
a) J.J. Thompson
b) E. Rutherford
c) Neils Bohr
5. For each of the following give:
i) atomic number
ii) mass number
iii) number of electrons
iv) number of protons
v) number of neutrons
vi) draw a Bohr diagram
12
a) 6 C
56
b) 26 Fe
235
c) 92 U
6. List the three main groups of elements, and list the characteristic properties of each
group.
7. State the symbols for the following elements:
(a) Helium
(b) Strontium (c) Fluorine
(e) Magnesium (f) Carbon
(g) Argon
(d) Bromine
8. Name the following elements:
(a) Cl (b) Na (c) Xe (d) Mo (e) Ba (f) Be (g) Mn (h) S
9. Draw electron dot diagrams for elements which have the following atomic
numbers: (Lewis Diagrams)
(a) 4
(b) 7 (c) 16 (d) 19
10. Explain and illustrate the variation of the following in the Periodic Table:
(a) ionization energy (b) electron affinity (c) atomic radius
11. For the following elements: (a) state if they tend to gain or lose electrons
(b) how many electrons are gained or lost.
(a) H (b) Na (c) Cl (d) Mg (e) S (f) Ne
3
12. Explain
(a) chemical bond (b) ionic bond (c) covalent bond
(d) polar covalent bond (e) electronegativity
(f) oxidation number (g) valence electrons (h) Octet rule
13. For each of the following combination of elements:
(a) use the electronegativity values to predict the type of bonding
(b) Draw the Lewis Diagrams
(c) Indicate the polarity if applicable
(d) Write the chemical formula
(i) Na and Cl
(b) Sr and F
(c) H2 and O2 (d) I and Br
14. Explain the term ACTIVITY SERIES with respect to alkali metals and
halogens
Chemical Reactions
1. Balance the following chemical equations:
(a) __H3PO4(aq) + __KOH(aq)----> __K3PO4(aq) + __H2O(l)
(b) __N2(g) + __H2(g)----> __NH3(g)
(c) __SF4(s) + __H20(l)----> __SO2(g) + __HF(aq)
(d) __Al2O3(s) + __H2(g)----> __Al(s) + __H2O(l)
(e) __HNO3(aq)----> __H2O(l) + __NO2(g) + __O2(g)
2. Name the type of chemical reaction that takes place in each example of question 1.
3. Explain the following: (i) endothermic reaction (ii) exothermic reaction (iii) aq
(iv) s (v) g (vi)
4. Write the correct formula for the following chemical compounds:
(a) sodium hydroxide (b) ferric oxide (c) iron (III) chloride
(d) aluminum acetate (e) potassium chlorate (f) tin (IV) chloride
(g) lead (II) carbonate
5. Write the correct name for the following chemical formulas:
(a) SiCl4 (b) Hg2O (c) HClO2 (d) NaH2PO3 (e) (NH4)3PO4 (f) BaSO4
Electron Configurations
1. The total number of orbitals containing electrons in the vanadium atom (23V) is
a)
4
b) 7
c)
12
d) 13
e)
23
4
2. The number of half-filled orbitals in the valence shell of an oxygen atom ( 8O ) in its
ground state is
a)
1
b) 2
c)
3
d) 0
e)
4
3. The shape of a PF3 molecule is best described as:
a) linear
b) bent
c) pyramidal
d) tetrahedral
e) planar triangular
4. Indicate the quantum numbers for each of the orbitals of the sub-levels indicated in the
following chart:
n
l
m
a) 3 d sub-level
b) 5 s sub-level
5. Element "X" is in the same family of elements as 16S.
a) Draw a Lewis (electron dot) diagram for element "X"
b) When element "X" forms an ion, what will be its charge?
6.
7.
Draw an energy level diagram for 33 As.
Using the format 1s2 2s2 , etc., write the electronic configuration for
35 Br