Download Exam2 Review

Exam #2 Review
Chapter 6
6.3
Heat can be determined by measuring temperature changes.
A.
Terminology.
1.
Boundary.
2.
System.
3.
Open system.
4.
Closed system.
5.
Isolated system.
B.
The heat an object gains or loses is directly proportional to its temperature change.
1.
Specific heat is an intensive property related to heat capacity.
2.
The algebraic sign of q is used to indicate the direct of heat flow.
6.4
Energy is absorbed or released during most chemical reactions.
A.
Exothermic reactions release heat; endothermic reactions absorb heat.
B.
Energy can be released by breaking weak bonds to form stronger ones.
6.5
Heats of reaction are measured at constant volume or constant pressure.
A.
Heat and work are both ways to transfer energy.
1.
First law of thermodynamics.
B.
Heats of combustion are determined using constant-volume calorimetry.
C.
Heats of reactions in solution are determined by constant-pressure calorimetry.
1.
Enthalpy.
2.
Enthalpy change.
6.6
Thermochemical equations are chemical equations that quantitatively include heat.
A.
Standard heat of reaction (ΔHº) is the enthalpy change for a reaction with all
reactants and products at standard state.
6.7
Thermochemical equations can be combined because enthalpy is a state function.
A.
Both the coefficients and direction of thermochemical equations can be adjusted.
B.
Enthalpy changes depend only on initial and final states, not on the path between
them.
C.
Enthalpy diagrams show alternative pathways between initial and final states.
1.
Enthalpy diagram.
D.
Predict any heat of reaction using Hess’s law.
6.8
Tabulated standard heats of reaction can be used to predict any heat of reaction using Hess’s
law.
Chapter 7
7.1
Electromagnetic radiation provides the clue to the electronic structures of atoms.
A.
Electromagnetic radiation can be described as a wave or as a stream of photons.
1
B.
C.
1.
Electromagnetic wave.
2.
Amplitude.
3.
Frequency.
4.
Wavelength.
5.
Speed of light.
Electromagnetic waves are categorized by frequency.
1.
Visible light.
Electromagnetic radiation can be viewed as a stream of photons.
7.2
Atomic line spectra are evidence that electrons in atoms have quantized energies.
A.
A simple pattern of lines in the spectrum of hydrogen suggests a simple explanation
for atomic spectra.
1.
Rydberg equation.
B.
The energy of electrons in atoms is quantized.
1.
Energy levels.
C.
The Bohr model explains the simple pattern of lines seen in the spectrum of
hydrogen.
1.
Quantum number.
2.
Ground state.
D.
The Bohr model fails for atoms with more than one electron.
7.3
Electrons have properties of both particles and waves.
A.
Diffraction provides evidence that electrons have wave properties.
B.
Bound electrons have quantized energies because they behave like standing waves.
1.
Traveling waves.
2.
Standing waves.
3.
Electron waves are represented by wave functions.
C.
Electron waves in atoms are called orbitals.
1.
The principle quantum number, n.
2.
The secondary quantum number, l.
3.
The magnetic quantum number, ml.
D.
The whole picture.
7.4
Electron spin affects the distribution of electrons among orbitals in atoms.
A.
Electrons behave like tiny charges that can spin in one of two directions.
1.
Electron spin.
2.
Spin quantum number, ms.
B.
No two electrons in an atom have identical sets of quantum numbers.
C.
Atoms with unpaired electrons are weakly attracted to magnets.
1.
Paramagnetic.
2.
Diamagnetic.
7.5
The ground state electron configuration is the lowest energy distribution of electrons among
2
orbitals.
A.
Electron configurations are built up by filling lowest energy orbitals first.
1.
Aufbau principle.
2.
How s – orbitals fill.
3.
Filling p and d – orbitals.
4.
Hund’s rule.
7.6
Electron configurations explain the structure of the periodic table.
A.
The periodic table is a guide for predicting electron configurations.
B.
Electron configurations can be abbreviated using noble gas core configurations.
C.
Chemical properties of the representative elements depend on valence shell electron
configurations.
1.
Outer shell.
2.
Core electrons.
D.
Configurations for transition and rare earth elements are sometimes unexpected.
7.7
Quantum theory predicts the shapes of atomic orbitals.
A.
Describing an electron’s position.
1.
Uncertainty principle.
2.
Electron cloud.
3.
Electron density.
B.
s Orbitals are spherical; p orbitals have two lobes.
1.
Node.
2.
Nodal plane.
3.
Orbitals in a p subshell are oriented at 90o to each other.
C.
Four of the five d orbitals in a d subshell have the same shape.
7.8
Atomic properties correlate with an atom’s electron configuration.
A.
Effective nuclear charge is the positive charge “felt” by outer electrons.
B.
Atomic and ionic sizes increase with increasing n and decreasing effective nuclear
charge.
1.
Atomic size varies periodically.
2.
Ion size show the same trends as atom sizes, but anions are larger and cations
are smaller than their parent atoms.
C.
Energy changes are associated with the gain or loss of electrons by atoms.
1.
The ionization energy is the energy required to remove an electron from an
atom or ion.
2.
Large atoms have lower ionization energies.
a.
First ionization energy.
b.
Diagonal relationship.
3.
Noble gas configurations are extremely stable.
4.
Electron affinity is energy released or absorbed when a particle gains an
electron.
3
4