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CEM 141 EXAM 3 MSU
- ANS-Lewis Dot Structure for H2O
-Hard
-Conduct electricity
-Shiny
-React w/water
-Malleable - ANS-What properties do metals have?
-Present in all substances
-Temporary fluctuating dipoles
-Depends on size, surface area, and shape of molecule - ANS-London Dispersion Forces
-Present in polar substances (along with LDF)
-Typically stronger than LDF - ANS-Dipole-Dipole Interactions
-Size of an atom
-Size of positive charge - ANS-Ionization energies are affected by
-Small atoms have higher ionization energies
-They are inversely related - ANS-Periodic Trends
# of protons. - ANS-Atomic # =
1. Draw Lewis Structure
2. Determine the electron pair geometry
3. Determine molecular shape
4. Determine the bond polarities
5. Add up the bond polarities
6. Figure out the molecular polarity. - ANS-How to determine molecular polarity?
1. Group number = How many valence electrons
2. For cations = (+) Remove electrons
3. For anions = (-) Add electrons
4. use 2 electrons for each atom - ANS-Lewis Structure
1) Molecular Formula
2) Lewis Structure
3) Electron Pair Geometry
4) Molecular Shape
5) Identification of bond properties
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6) Identification of molecular polarity
7) Deduce type and relative strength of IMFs
8) Predict properties - ANS-Structure Properties
3 sp2 orbitals; trigonal planar; sigma bond - ANS-Bonding in Graphite
A heavier nucleus is broken a part to form lighter, more stable nuclei energy. - ANS-Fission
A negatively charged ion, formed when non-metals gain electrons, change usually corresponds
to gain of electrons to next filled shell. - ANS-Anion
A positively charged ion, formed when metals lose electrons w/ low electronegativity, always
requires an input of energy. - ANS-Cation
Ability of an element to attract electrons to another electron. - ANS-Electronegativity
Ability of an element to attract electrons to itself in a bond. - ANS-Electronegativity
Are between a metal and non-metal. - ANS-Ionic Bonds -
Assume all centers of electrons density repel each other and that there is a minimum energy
arrangement that the atom will naturally take up. - ANS-Valence Shell Electron Pair Repulsion
(VSEPR)
Atomic orbitals overlap to form a bond. - ANS-Valence Bond
Bonding in carbon compound bonds to C,H,O,N,S,P. - ANS-Heterogeneous Compounds
C - sp hybridized
One sigma bond
Two pi bonds - ANS-Triple Bonds
Contains a metal and a non-metal; metals form cations and non metals form anions. -
ANS-Simple Ionic Compound
Decreases. - ANS-Does electronegativity increase or decrease down a group?
Each carbon forms 4 bonds to 4 identical carbons; tetrahedral; sp3 - ANS-Binding in Diamond
Electrons shared equally. - ANS-Non polar covalent bond =
Electrons shared unequally. - ANS-Polar covalent bond =
Electrons transferred. - ANS-Ion-Ion Interactions
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141 EXAM 3 MSU.pdf#######################################
CEM 141 EXAM 3 MSU
- ANS-Lewis Dot Structure for H2O
-Hard
-Conduct electricity
-Shiny
-React w/water
-Malleable - ANS-What properties do metals have?
-Present in all substances
-Temporary fluctuating dipoles
-Depends on size, surface area, and shape of molecule - ANS-London Dispersion Forces
-Present in polar substances (along with LDF)
-Typically stronger than LDF - ANS-Dipole-Dipole Interactions
-Size of an atom
-Size of positive charge - ANS-Ionization energies are affected by
-Small atoms have higher ionization energies
-They are inversely related - ANS-Periodic Trends
# of protons. - ANS-Atomic # =
1. Draw Lewis Structure
2. Determine the electron pair geometry
3. Determine molecular shape
4. Determine the bond polarities
5. Add up the bond polarities
6. Figure out the molecular polarity. - ANS-How to determine molecular polarity?
1. Group number = How many valence electrons
2. For cations = (+) Remove electrons
3. For anions = (-) Add electrons
4. use 2 electrons for each atom - ANS-Lewis Structure
1) Molecular Formula
2) Lewis Structure
3) Electron Pair Geometry
4) Molecular Shape
5) Identification of bond properties
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6) Identification of molecular polarity
7) Deduce type and relative strength of IMFs
8) Predict properties - ANS-Structure Properties
3 sp2 orbitals; trigonal planar; sigma bond - ANS-Bonding in Graphite
A heavier nucleus is broken a part to form lighter, more stable nuclei energy. - ANS-Fission
A negatively charged ion, formed when non-metals gain electrons, change usually corresponds
to gain of electrons to next filled shell. - ANS-Anion
A positively charged ion, formed when metals lose electrons w/ low electronegativity, always
requires an input of energy. - ANS-Cation
Ability of an element to attract electrons to another electron. - ANS-Electronegativity
Ability of an element to attract electrons to itself in a bond. - ANS-Electronegativity
Are between a metal and non-metal. - ANS-Ionic Bonds -
Assume all centers of electrons density repel each other and that there is a minimum energy
arrangement that the atom will naturally take up. - ANS-Valence Shell Electron Pair Repulsion
(VSEPR)
Atomic orbitals overlap to form a bond. - ANS-Valence Bond
Bonding in carbon compound bonds to C,H,O,N,S,P. - ANS-Heterogeneous Compounds
C - sp hybridized
One sigma bond
Two pi bonds - ANS-Triple Bonds
Contains a metal and a non-metal; metals form cations and non metals form anions. -
ANS-Simple Ionic Compound
Decreases. - ANS-Does electronegativity increase or decrease down a group?
Each carbon forms 4 bonds to 4 identical carbons; tetrahedral; sp3 - ANS-Binding in Diamond
Electrons shared equally. - ANS-Non polar covalent bond =
Electrons shared unequally. - ANS-Polar covalent bond =
Electrons transferred. - ANS-Ion-Ion Interactions
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