Chap 1-3 Review

Chapter #1-3 Review
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Define matter and energy.
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Summarize the four point in the Kinetic Molecular Theory
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What are the four states of matter?
Draw a diagram and label the phase transitions between the states.
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Solid, liquid, gas, plasma
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Give one example of a qualitative property of matter.
Give one example of a quantitative property of matter.
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Qualitative - “what type?” - blue, green, tall, short
Quantitative - “How much?” - 6’1”, 170 lbs, 16 seconds
Matter - anything that has a rest mass and occupies a volume
Energy - anything that is not matter but can cause a change in matter
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two categories, kinetic and potential
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List the main points of each atomic theory.
Dalton, Thomson, Rutherford and Bohr.
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Dalton - Atoms are hard featureless spheres. Each element has a unique kind of
atom. Combinations of atoms make compounds
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Rutherford - Electrons are small negatively charged particles that orbit a small
massive positively charged nucleus. Atoms are mostly empty space.
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Bohr - Electrons are located in shells. Electrons are negatively charged particles
located in shells surrounding a small dense positively charged nucleus.
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Give the name, charge, location and mass for each subatomic particle.
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Proton!!
+1!
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nucleus!
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1.0 amu
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Neutron!
0!
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nucleus!
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1.0 amu
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Electron!
-1!
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shells! !
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1/1834 amu
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A previously unknown element has the following information:
Atomic number = 117
Atomic mass = 290
Describe this element in terms of number of each subatomic particle and
predict the most likely ionic charge.
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# protons = 117!
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# neutrons = 290-117 = 173!!
# electrons = 117
Thomson - Atoms contain small negative particles called electrons. The
background contains a postive charge to maintain neutrality.
In the halogen column therefore
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Ionic Charge = -1
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Draw the Bohr model diagrams for the following species (**watch the charge**)
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Mg!
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N!
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P3-!
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Na1+!
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S2-
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In terms of electrons, what is the primary difference between ionic and
covalently boned compounds?
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Covalent - electrons are shared between the two nuclei
Ionic - one or more electrons are transferred from the metal atom to the
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non-metal atom creating ions, the ions are then electrostaticallt attracted
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to each other.
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Explain why elements want to form simple ions. What is the goal?
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All elements attempt to get a noble gas configuration of electrons. For very small
elements they try to get 2 electrons like helium, for all larger elements the goal is 8
electrons in the valence shell.
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Name the following compounds
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12)
ICl3 !
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N2O3! !
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SO3! !
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SeF2! !
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Cd3N2! !
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Fe3As2!!
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Ag2CO3
Ca3P2! !
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Zn(NO3)2!
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PbCrO4!
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Pt(CH3COO)4!
Iodine trichloride
Dinitrogen trioxide
Sulfur trioxide
Selenium difluoride
Cadmium (II) nitride
Iron (III) arsenide
Silver carbonate
Calcium phosphide
Zinc nitrate
Lead (II) chromate
Platinum (IV) acetate
Give the formula for each compound (**watch endings**)
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b)
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d)
e)
f)
g)
h)
carbon diarsenide
tetrasufur dinitride
nitrogen trichloride
calcium fluoride
technetium (IV) sulphide
tin (IV) carbonate
antimony (V) nitrate
manganese (II) chlorite
CAs2
S 4N 2
NCl3
CaF2
TcS2
Sn(CO3)2
Sb(NO3)5
Mn(ClO2)2
13)
List four difference evidences for a chemical change.
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New colour! !
New odour! !
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Change of phase (eg solid or gas formed)
New texture
14)!
Classify each reaction in terms of;
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chemical versus physical! !
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Frying an egg!
chemical & endothermic
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Burning natural gas in a furnace! chemical & exothermic
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Lifting a text book from the floor to the table!
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physical & endothermic
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Two solutions are mixed and the resulting mixture begins to glow green
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chemical & exothermic
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A candle burning!
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Recharging the battery on a cellphone!
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exothermic versus endothermic
chemical & exothermic
chemical & endothermic