CHEMISTRY TEST REVIEW - ANSWERS
PERIODIC TABLE, CHEMICAL BONDING, LEWIS DOT DIAGRAMS, &
VSEPR
GENERAL NOTES on TEST:
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Test Format may include multiple choice, matching, true/false, calculations, drawing
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You may use a calculator
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You may have one (1) 3 x 5 index card and can use both sides for key definitions, examples,
formulas, periodic table reminders, etc.
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You may use a periodic table – not the color coded one
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NO – THE TEST WILL NOT LOOK JUST LIKE THE REVIEW
1.
Be able to fill in a fictitious periodic table based on criteria related to the actual periodic table.
For example – how knowing the number protons or electrons, energy level, electron
configuration, family characteristics, relationship to other clues
2.
Be able to identify ionic, covalent, polar covalent, and metallic bonds.
Which ions bond together
Ionic – anions and cations
Covalent – anions
Metallic -- cations
Which generic element families (non-metals, metals) bond together
Ionic – metals and non-metals
Covalent – non-metals
Metallic – metals
How are ionic, covalent, polar covalent, and metallic bonds similar?
Involve valence electrons, form from more than one atom (of same or different
element), Lewis Dot Diagrams look the same
How are ionic, covalent, polar covalent, and metallic bonds different?
Ionic electrons transfer, shared in covalent, metallic free flowing. Ionic and
metallic form solids… covalents often liquids and gases and form double or triple
bonds the other two do not. Naming convention is different.
3,
Calculate the difference in electronegativity when the following bonds form knowing ranges for
each
Ionic
Greater than 1.7
Polar Covalent
0.3 – 1.7
Non-Polar Covalent
4.
0 – 0.3
Identify examples of ionic, covalent, and metallic bonds
For Example
NaS2 ionic CO covalent NiCd metallic
5.
NH3
covalent
Fe2O3 ionic
Know that non-metals and hydrogen only form single covalent bonds and that double and triple
covalent bonds occur (for example – carbon based materials such as carbon dioxide, certain
fuels)
Be able to draw Lewis Dot Structures for individual elements
Potassium
Fill one e- on each side
before doubling up
Bromine
K
Br
Be able to draw Lewis Dot Structures for molecules. Identify bond pairs and lone pairs.
NO2
MgF --
O–N–O
can form Reasonance Structure by bonding to
Oxygen on right instead
You are on your own for
these three
PO3
LiF
Be able to identify a reasonance structure -- See NO2 above
Example - SO3
This reasonance structure was on the VSEPR graphic organizer we did in
class. Double bond can form between sulfur atom and any one of the three oxygen atoms.
6.
Know how chemical bonds form
Ionic - ____transfer______________ electrons
Covalent - ___share____________ electrons
Metallic – electrons are ____free________ __flowing______________
7.
Identify properties of chemical bonds
Ionic – valence electrons are transferred between metals (cations) and non-metals
(anions). Form crystalline structures, solids. Can be conductors of electricity.
Covalent – valence electrons are shared between non-metals (anions). Usually gases
or liquids. Don’t conduct electricity. Form higher energy double or triple bonds
Metallic – valence electrons are free flowing (sea or cloud of electrons). Solid
Or crystalline structure. Conduct electricity easily, shiny
8.
Know why polarity is important and cite a real world example of it
Polarity is tendancy of electrons to be attracted towards one atom over another which gives a
molecule solvent properties to attract other molecules. Water is an example of a great solvent.
9.
What do the initials VSEPR stand for?
Valence Shell Electron Pair Repulsion
Explain the VSEPR Theory.
Since like charges repel, electrons will repel each other to the greatest distance
(angular degree) possible.
Be able to draw or construct linear, trigonal planar, and tetrahedral VSEPR for various
molecules. Identify the angles between pairs in the proper number of degrees.
For example –
CO2
BF3
Linear
Trigonal planar
180° angle
120° angles
CF4
Tetrahedral 109.5° angles