MSU CEM 141 FINAL EXAM QUESTIONS WITH
COMPLETE SOLUTIONS| LATEST UPDATE
Doppler Effect Frequency increases, creating a higher pitch when moving toward
Frequency decreases, creating a lower pitch when away.
E = mc2 Binding energy, the energy released when mass is converted to energy (nuclear
reaction).
Effective Nuclear Charge = Protons - Core Electrons
Increases across the row, decreases down the group (as atomic radius decreases)
How tight the electrons are being attracted to the nucleus.
electromagnetic force attraction/repulsion between objects with electrical charge
Fe=Q1Q2/r^2
Electronegativity Ability of an element to attract electrons to another electron.
Electronegativity Ability of an element to attract electrons to itself in a bond.
Emergent Properties When atoms interact to form larger molecules/structures, like
melting/boiling point.
energy can be transferred or transformed
Energy is _____ to the surroundings when atoms attract each other released
Energy of light equation? E = hV.
Energy of Wave (J) Increases as frequency increases and as wavelength decreases. Highest: x-
ray
,energy units joule (kg/m^2s^2) and calories.
Everything in the universe is moving away from us with ____ speed. Increasing
Evidence: Ejection of electrons when light shines on a metal surface.
Reasoning: _______________ Ejection of electrons is only observed when the light has
frequencies above a threshold value.
force (types) gravitational, electromagnetic, strong, weak
Formal Charge = Valence electrons - # of bonds - non bonded electrons
Formal Charge on OH-? O: FC = 6 - 1 - 6 = -1.
Forming bonds releases... Energy.
Frequency (V) The number of wavefronts per second. Highest: x-ray
Gas LDF and covalent bonds are overcome by energy.
Gas to Liquid to Solid Phase change: releases energy, energy released to surroundings, attractions
formed between molecules.
generic formula for a hydrocarbon containing "n" carbon atoms? CnH2n+2
Gold foil experiment -most particles went straight through
-every once in awhile particles were deflected
-1/8000 particles bounced back
-led to model of atom; small, dense, positively charged nucleus
Graphite Allotrope of Carbon with high melting point, soft, slippery, grey, shiny, conducts
electricity.
gravitational force attraction between objects that have mass. requires 2+ objects
Fg=Gm1m2/r^2
Greek philosophers atomic theory -first atomic theory
-elements: earth, fire, water, air
-constantly in motion
-made of mostly empty space
h Planck's constant, the energy of a photon.
H Bond In H-H only the bonding MO is occupied, leading to net stabilization of the
interaction
, Breaking bond: enough energy has to be added to raise an electron to the antibonding orbital.
Heisenberg Uncertainty Principle Principle states that we can't accurately measure both the
position and the energy of a small particle (electron)
Bohr's model did - why its wrong.
Heterogeneous Compounds Bonding in carbon compound bonds to C,H,O,N,S,P.
How is absorption and emission different from photoelectric effect? In the photoelectric
effect, an atom absorbs a photo resulting in the ejection of an electron.
How is the temperature of a phase change related to different elements? the temperature of a
phase change depends on the strength of the intermolecular forces. stronger force=higher
temperature
how many atoms are naturally occurring? 91 naturally occurring elements
How many core electrons and valence electrons does N have? 2 core, 5 valence.
How many core electrons and valence electrons does Si have? 10 core, 4 valence.
How many electrons are emitted if the light is below it's threshold frequency no matter the
intensity? None.
How many electrons can fit in one p orbital? Two.
How many electrons can fit in one set of p orbitals? Six.
How many orbitals are in the electron cloud of one atom? All.
How many valence electrons do elements in group 3A have? 3.
How to determine molecular polarity? 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.
Hund's Rule Rule that electrons occupy orbitals of the same energy singly until they have to
pair up.
Hybridized bonds One s and three p orbitals combine to create sp3 orbitals, create strong
sigma bonds (like in diamonds) between atoms.
COMPLETE SOLUTIONS| LATEST UPDATE
Doppler Effect Frequency increases, creating a higher pitch when moving toward
Frequency decreases, creating a lower pitch when away.
E = mc2 Binding energy, the energy released when mass is converted to energy (nuclear
reaction).
Effective Nuclear Charge = Protons - Core Electrons
Increases across the row, decreases down the group (as atomic radius decreases)
How tight the electrons are being attracted to the nucleus.
electromagnetic force attraction/repulsion between objects with electrical charge
Fe=Q1Q2/r^2
Electronegativity Ability of an element to attract electrons to another electron.
Electronegativity Ability of an element to attract electrons to itself in a bond.
Emergent Properties When atoms interact to form larger molecules/structures, like
melting/boiling point.
energy can be transferred or transformed
Energy is _____ to the surroundings when atoms attract each other released
Energy of light equation? E = hV.
Energy of Wave (J) Increases as frequency increases and as wavelength decreases. Highest: x-
ray
,energy units joule (kg/m^2s^2) and calories.
Everything in the universe is moving away from us with ____ speed. Increasing
Evidence: Ejection of electrons when light shines on a metal surface.
Reasoning: _______________ Ejection of electrons is only observed when the light has
frequencies above a threshold value.
force (types) gravitational, electromagnetic, strong, weak
Formal Charge = Valence electrons - # of bonds - non bonded electrons
Formal Charge on OH-? O: FC = 6 - 1 - 6 = -1.
Forming bonds releases... Energy.
Frequency (V) The number of wavefronts per second. Highest: x-ray
Gas LDF and covalent bonds are overcome by energy.
Gas to Liquid to Solid Phase change: releases energy, energy released to surroundings, attractions
formed between molecules.
generic formula for a hydrocarbon containing "n" carbon atoms? CnH2n+2
Gold foil experiment -most particles went straight through
-every once in awhile particles were deflected
-1/8000 particles bounced back
-led to model of atom; small, dense, positively charged nucleus
Graphite Allotrope of Carbon with high melting point, soft, slippery, grey, shiny, conducts
electricity.
gravitational force attraction between objects that have mass. requires 2+ objects
Fg=Gm1m2/r^2
Greek philosophers atomic theory -first atomic theory
-elements: earth, fire, water, air
-constantly in motion
-made of mostly empty space
h Planck's constant, the energy of a photon.
H Bond In H-H only the bonding MO is occupied, leading to net stabilization of the
interaction
, Breaking bond: enough energy has to be added to raise an electron to the antibonding orbital.
Heisenberg Uncertainty Principle Principle states that we can't accurately measure both the
position and the energy of a small particle (electron)
Bohr's model did - why its wrong.
Heterogeneous Compounds Bonding in carbon compound bonds to C,H,O,N,S,P.
How is absorption and emission different from photoelectric effect? In the photoelectric
effect, an atom absorbs a photo resulting in the ejection of an electron.
How is the temperature of a phase change related to different elements? the temperature of a
phase change depends on the strength of the intermolecular forces. stronger force=higher
temperature
how many atoms are naturally occurring? 91 naturally occurring elements
How many core electrons and valence electrons does N have? 2 core, 5 valence.
How many core electrons and valence electrons does Si have? 10 core, 4 valence.
How many electrons are emitted if the light is below it's threshold frequency no matter the
intensity? None.
How many electrons can fit in one p orbital? Two.
How many electrons can fit in one set of p orbitals? Six.
How many orbitals are in the electron cloud of one atom? All.
How many valence electrons do elements in group 3A have? 3.
How to determine molecular polarity? 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.
Hund's Rule Rule that electrons occupy orbitals of the same energy singly until they have to
pair up.
Hybridized bonds One s and three p orbitals combine to create sp3 orbitals, create strong
sigma bonds (like in diamonds) between atoms.
