Title: Chemistry 1301A (WebStraw)
Tags: Chem1301::Chapter3 Chem1301::Chapter2 Chem1301::Chapter4 Chem1301::Chapter5

Q: The intensity of an electromagnetic wave is proportional to [...] of its amplitude
A: the square

Q: The [...] series describes the discrete wavelengths of light in the visible region of the EM spectrum emitted by excited hydrogen
A: Balmer

Q: The [...] series describes the wavelengths of light in the [...] region of the EM spectrum emitted by excited hydrogen
A: Paschen; infrared

Q: The [...] series describes the wavelengths of light in the [...] region of the EM spectrum emitted by excited hydrogen
A: Lyman; ultraviolet

Q: The probability of an electron being at a point is proportional to [...] at that point
A: the square of its wavefunction

Q: The principal (n) quantum number describes the [...] of an electron
A: energy level

Q: The azimuthal (l) quantum number describes the [...] of an electron
A: orbital shape

Q: The magnetic (m(l)) quantum number describes the [...] of the orbital
A: XYZ-axis relative orientation

Q: How does the range of azimuthal quantum number (l) values relate to the principal quantum number (n)?
[...]
A: 0≤ l ≤ (n-1)

Q: How does the range of magnetic quantum number (m) values relate to the azimuthal quantum number?
[...]
A: -l ≤ m ≤ l

Q: As the principal quantum number increases for the same orbital shape, the number of [...] nodes increases
A: radial

Q: How is the number of radial nodes related to the principal quantum number (n)?
[...]
A: number of radial nodes = n-1

Q: Different orbitals in the same energy level differ in the number of [...] nodes
A: angular

Q: State the Aufbau principle
[...]
A: Electrons fill orbitals of lower energy first

Q: State Hunds rule
[...]
A: Electrons enter degenerate empty orbitals with the same spin before doubling up

Q: State the Pauli exclusion principle
[...]
A: Electrons in the same orbital must have opposite spins

Q: What are isoelectric species?
[...]
A: Chemical species with the same electronic configuration

Q: What term describes two chemical species with the same electronic configuration?
[...]
A: Isoelectric

Q: A region of space with a 0% probability of containing an electron is called a [...]
A: node

Header: What orbital shape is shown in the following image (s, p, d,f)?

Header: Describe the following shape and orientation of the following orbital

Header: Describe the following shape AND orientation of the following orbital

Q: How many angular nodes are in an d orbital?
[...]
A: 2

Q: How many angular nodes are in an s orbital?
[...]
A: 0

Q: How many angular nodes are in a p orbital?
[...]
A: 1

Q: Ionic bonding atoms form three dimensional structures called [...] in which each ion is connectet to multiple others
A: crystal lattices

Q: What law can be used to deduce the strength of an ionic interaction between charged atoms?
[...]
A: coulombs law
Extra: Depends on the charge and distance between atoms! Pay attention to how each property influences ionic strength based on Coulombs law.

Q: How is the formal charge on an atom calculated?
[...]
A: formal charge=valence electrons-electrons owned
Extra: ie. For O2, the formal charge on one oxygen is
C(f) = n(valence) - n(owned) = 6-6 = 0

Q: What term describes the difference between an atoms expected number of valence electrons and the number of electrons it effectively possesses in a molecule?
[...]
A: Formal Charge

Q: The octet rule applies to which periods in the periodic table?
[...]
A: Period 2 (and period 1 elements may have a maximum of 2 electrons)

Q: Elements from which period(s) are capable of carrying an expanded octet?
[...]
A: n ≥ 3

Q: The best Lewis structures for a molecule with respect to formal charges tend to have:
1. [...]
2. [...]
A: formal charges consistent with electronegativities; low numbers of non-zero formal charges

Q: Resonance structures are those that differ only in [...]
A: the location of multiple bonds and electrons

Q: What are structures that differ only in the location of double bonds are electrons?
[...]
A: Resonance structures

Q: The average bond order of an atom is the average [...]
A: number of bonds between specific atoms

Q: In AXE notation, the A represents the [...]
A: central atom

Q: In AXE notation, the X represents the [...]
A: ligands

Q: In AXE notation, the E represents the [...]
A: electron pairs

Header: Name the molecular shape according to VSEPR theory

Q: According to VSEPR theory, what exerts a greater force on neighboring electron domains: bonds or lone pairs?
[...]
A: Lone pairs

Q: According to VSEPR, a molecule with 2 regions of electron density has a [...] geometry
A: linear

Q: According to VSEPR, a molecule with 3 regions of electron density has a [...] geometry
A: trigonal planar

Q: According to VSEPR, a molecule with 4 regions of electron density has a [...] geometry
A: tetrahedral

Q: According to VSEPR, a molecule with 5 regions of electron density has a [...] geometry
A: trigonal bipyrimidal

Q: According to VSEPR, a molecule with 6 regions of electron density has a(n)[...] geometry
A: octahedral

Q: In a trigonal bipyramidal shape, the electron domains separated by 120 degrees from eachother are termed [...]
A: equatorial

Q: In a trigonal bipyramidal shape, the electron domains separated by 180 degrees from eachother are termed [...]
A: axial

Q: In a dot-line-wedge diagram, a wedge refers to a bond coming [...] the page
A: out of

Q: In a dot-line-wedge diagram, a dashed wedge refers to a bond coming [...] the page
A: into

Q: Hydrogen bonds can only form from a hydrogen bonded to a [...], and an electron pair from another of these elements
A: nitrogen, oxygen, or fluorine

Q: Dispersion forces occur due to the formation of [...]
A: temporary dipoles

Q: The strength of dispersion forces is most strongly influenced by the [...] of each molecule
A: surface area (available for temporary dipoles to form)

Q: What property strongly influences the melting point of a substance but NOT its boiling point?
[...]
A: molecular symmetry

Q: In valence bond theory (hybridization model), pi bonds are created by [...] orbitals
A: p

Q: [...] bonds are formed by the [...] overlap of two p orbitals
A: Pi; sideways

Q: A triple bond is composed of [...] sigma bond and [...] pi bonds
A: 1; 2

Q: The HOMO in molecular orbital theory stands for the [...]
A: highest occupied molecular orbital

Q: The LUMO in molecular orbital theory stands for the [...]
A: Lowest unoccupied molecular orbital

Q: The equation for the bond order in MO theory is bond order = [...]
A: (bonding MOs - antibonding MOs)/2

Q: A [...] species is [...] a magnetic field
A: paramagnetic; attracted to

Q: A [...] species is [...] a magnetic field
A: diamagnetic; not attracted to

Q: A [...] species must have one or more [...]
A: paramagnetic; unpaired electrons

Q: A [...] species must have [...]
A: diamagnetic; no unpaired electrons

Q: The fusion of two atomic orbitals always yields a(n) [...] MO and a(n) [...] MO
A: bonding; antibonding

Q: A [...] is defined as a polyatomic structure with atleast one [...]
A: complex; transition metal ion/atom.

Q: A charged complex is referred to as a [...]
A: ionic complex/complex ion

Q: A [...] is any atom or molecule that is [...]
A: ligand; bound to a central metal ion

Q: A [...] atom is the atom of a ligand that is [...].
A: donor; directly bound to the metal centre

Q: The [...] of a ligand refers to the [...] that it has
A: denticity; number of donor atoms

Q: A [...] ligand is one in which [...]
A: chelating; multiple donor atoms binding the same metal centre

Q: [...] isomers are complexes with [...]
A: Linkage; the same ligands but differing in the donor atom

Q: [...] isomers are complex salts that differ only in [...]
A: Ionization; the anion in complex with the metal

Q: By convention, the metal centre and all of its ligands should be recorded in [...]
A: square brackets

Q: [...] isomers are salts composed of two complex ions differing only [...]
A: Coordination; in the location of the central metal ions

Q: What is/are the possible stereochemistries of complexes with a coordination number of 4?
[...]
A: Square planar or tetrahedral

Q: What two isomers are possible in a complex with coordination number 4 and square planar stereochemistry?
1. [...]
2. [...]
A: cis - identical ligands separated by 90 degrees); trans - identical ligands separated by 180 degrees

Q: What stereochemistries can be possessed by a complex with coordination number 5?
[...]
A: square pyrimidal OR trigonal bipyrimidal

Q: What is the most common coordination number amongst transition metal complexes?
[...]
A: 6

Q: What are the angles between identical ligands in a mer isomer?
[...]
A: All 90 degrees

Q: What are the angles between identical ligands in a fac isomer?
[...]
A: 90, 90, 90

Q: What are all 3 angles between identical ligands in an octahedral complex?
[...]
A: 90, 90, 180

Q: During the mond process, nickel is reacted with [...] to form a highly [...] compound
A: carbon monoxide; volatile

Q: What is the purpose of the Mond process?
[...]
A: To separate nickel from impurities

Q: A [...] complex describes a metal complex with a [...] ligand
A: metal carbonyl; CO

Q: What is the below structure called?
[...]
A: porphyrin

Q: What is the central metal ion in heme?
[...]
A: Iron

Q: Hemoglobin is composed of [...] globin polypeptides and [...] heme group
A: 4; 1

Q: [...] are a pair of molecules that are [...]
A: Enantiomers; non-superimposible mirror images of eachother

Q: What 2 physical/chemical properties are different between a pair of enantiomers?
1. [...]
2. [...]
A: direction that polarized light is rotated; Chemical reactions with other chiral compounds

Q: What is a chiral/stereocentre?
[...]
A: Atom bonded to 4 different groups in tetrahedral shape

Q: An atom bonded to 4 different substituents in a tetrahedral arrangement is called a [...]
A: chiral/sterocenter

Header: Determine whether the given configuration is R or S

Q: A [...] is a 50-50 mixture of a pair of enantiomers
A: racemic mixture

Q: What term refers to a mixture of enantiomers in a 1:1 ratio?
[...]
A: racemic mixture

Q: The [...] enantiomer rotates plane-polarized light to the [...] is labelled
A: (+); right

Q: The [...] enantiomer rotates plane-polarized light to the [...] is labelled
A: (-); left

Q: Light that is all oscillating in the same plane is said to be [...]
A: plane-polarized