Chemistry Exam 3 Memorization
Space formed by overlapping orbitals can accommodate a maximum of_______ electrons and the electron must have____________ paired spins
(VB Theory) two Opposite
The greater the overlap. the ________ the bond, overlap depends on orbital __________ and direction
(VB theory) Stronger Shape
The spin quantum number represents the______________________________, what is the # for Cu
-1/2
What is the EN of noble gases?
0
This formula: O + E- --> O1- is EA__
1
Spx and Spy orbtials are in Ar. Which of the following statements are true 1.) They have the same energy 2.) They have the same orientation 3.) They have the same size
1 and 3
Shape of S orbital
1 x Circle
Steps for lewis structure
1.) # of valance electrons 2.) Arrange symmetrically(usually least EN in middle, never hydrogen) 3.) Make single bonds 4.) Fill outer elements with available valance electrons 5.) Any left over electrons must be put into central atoms 6.) Check to make sure middle atom has 8 electrons, if not make double and triple bonds 7.) Formal charge with the most zeroes for most favorable charge
What are the steps and energies in the born haber cycle?
1.) Li(s)-> Li(g) Endo 2.)1/2F2(g)--> F(g) Endo 3.)Li-> Li1+ + e- Endo 4.) F(g) + e- --> F-(g) Exo 5.) Li(s) + 1/2F2(g)--> LiF(s) Exo, formation of ionic solid
Single bond has an order of___________, double has an order of__________, and triple has an order of_______________
1.0 2.0 3.0
In group 2 and 3, what is the period order of increasing ionization energy
1A<3A<2A<4A<6A<5A<7A<8A
Complete electron config for chlorine?
1s2 2s2 2p6 3p2 3p5
O3- config
1s2 2s2 2p6 3s1
In determining electrostatic energy, determine________ first, then___________
Charge Size
Electrostatic energy formula
Charge of metal x charge of nonmetal / distance
_________________ bonds form when orbitals of two atoms overlap and a pair of electrons occupy the overlap region
Covalent (VB Theory)
Write out the condensed electron configuration for the following: Cr Cu Ag Au Mo Pd Nb Ru Rh
Cr: [Ar] 4s1 3d5 Cu: [Ar] 4s1 3d10 Ag: [Kr] 5s1 4d10 Au: [Xe] 6s1 4f14 5d10 Mo: [Kr] 5s1 4d5 Pd: [Kr] 4d10 Nb: [Kr] 5s1 4d4 Ru: [Kr] 4d7 5s1 Rh: [kr] 5s1 4d8
When electrons are removed, a cation is formed, and the atomic size______________
Decreases Na+1<Na
To move the electron density away from the middle of the element
Delocalize
Energy change when a nuetral atom attracts an electron.
Electron affinity
All of the Nonpolar shapes must have the same_________________to be nonpolar
Elements
The first Electron affinity is__________________, while the rest are_________________
Exothermic Endothermic(to overcome repulsions)
Diamagnetic elements are attracted by magnetic fields(T,F)
F
A series of sp2 orbitals can be thought of as one s orbital one-third of the time and two p orbitals two-thirds of the time(T,F)
F, why?
A set of sp orbitals can accommodate a maximum of six electrons(T,F)
F, why?
Delocalization creates space around the nucleus for stronger bonds and increases the overall energy of the element(T,F)
F; it lowers
Which element has these IE's in period 4 IE1= 900kj 1E2= 1134kj IE3= 1390kj IE4= 7896kj
Ga
The higher the energy level, the_____________ energy an electron has, the_______________ it is to remove an electron, the_____________ stable it is
Higher Easier Less
___________ rule states you fill in each electron configuration with one electron then return to fill in the rest
Hunds
All exceptions to octet rule
Hydrogen can have 2 Be only needs 4, can have more B only needs 6, can have more Nonmentals in period 3 and beyond can have more than 8 electrons in to fill octet
Which of the following statements concerning molecular orbital (MO) theory are correct? I. The Pauli Exclusion Principle is obeyed. II. Hund's rule is obeyed. III. A bonding molecular orbital is lower in energy than its parent atomic orbitals IV. The combination of two atomic orbitals creates one molecular orbital V. An antibonding molecular orbital is lower in energy than its parent atomic orbitals
I, II, III
All Trends Atomic size ____________ as you go down, and______________ as you go from right to left Electron affinity and ionization energy typically increase as you go___________ and from __________ to ____________ Metallic trends increase as you go_______ and from______________ Acidicity increases as you go _____________ and from ____________ to _________________-
Increases Increases Up Left to right Down Right to left Up Left to right
The amount of energy required to remove an electron from an atom is known as____________________
Ionization Energy (endothermic)
2 electron groups are_______________ the possible molecular arrangement is_________
Linear Linear
If two atomic orbitals form an MO, the resulting molecule will be____________ in energy than the original orbital. If they form an antibonding MO, the molecule will be____________in energy
Lower Higher
This theory considers the idea that all electrons in a molecule are delocalized over the entire region of a molecule, not just between each bond
Molecular Orbital Theory
Which of the following isn't addressed by molecular orbital theory?
Molecular geometry
When removing electrons in ion config u move from the highest__________ value, then from ________________
N FDPS
Inner core electrons are electrons in_________________ and_____________________
Noble gas config completed D and F orbitals
An EN difference of: .0 is____________ <.4 is________ .4 to 1.7 is_______ 1.7> is is__________
Nonpolar covalent Mostly nonpolar covalent Polar covalent Ionic
Formal Charge formula
Number of valance electrons of element - # of E around element - # of bonds, if can't get things to zero, make sure negative charge is most electromagnetic element and positive charge is least electromagnetic element
6 Electron groups are_____________ the possible molecular arrangements are____________________
Octahedral AX6, 90, 180, octahedral, not flat AX5E1; 90, Square pyramidal, not flat AX4E2, 90, square planar
An electron within an atomic orbital moves in a _______ function, oscillating from the positive to negative region if two electrons from separate atomic orbitals on separate atoms overlap when they were both in a positive region, the overlap would reinforce the attraction and a _________ MO would form, however, if the electrons are not in sync, the wave will cancel eachother, weakening the attraction and forming an _______________________ MO
Oscillating Bonding Antibonding
Electrons in the highest N value are the ______________ electrons
Outer
The more unpaired electrons, the more____________________
Paramagnetic
An atom with unpaired electrons is______________ and is attracted by an__________ field
Paramagnetic Magnetic
An unequal sharing of electrons is known as a____________ bond
Polar
For doing enthalapy of reaction with bond energies, the formula is______________ minus_____________
Reactants, products
What subshell does the angular momentum quantum number represent 0 1 2 3
S P D F
Valance electrons are the outer electrons in____ and _____, and the ___________ electrons in the d and f orbitals
S and P Non completed
Hybridization of linear molecules trigonal planar tetrahedral trigonal bipyramidal Octahedral
SP SP2 SP3 SP3D SP3D2
Created when as s and a p come together to delocalize the electron density around the central atom
SP orbital
Referred to as a single or localized bond in a compound, can be created with an overlap of two s orbitals or two SP orbitals or an sp orbital with an s orbital
Sigma bond
When dealing with isoelectric ions, the element with the most protons is the________________
Smallest
Molecular orbital theory addresses which of the following properties of molecules?
Spectral, Magnetic, Resonance
The angular momentum quantum number(L)describes the_________________, and the (L) for Cu is
Sublevel or subshell 2
A set of sp3 orbitals results from the mixing of one s orbital and three p orbitals. (T,F)
T
Ionic bonds are stronger than covalent bonds (T,F)
T
MO theory eliminates the need for resonance forms to depict polyatomic molecules.(T,F)
T
MOs are filled in order of their energy with paired electrons having opposite spins.(T,F)
T
The molecular orbital theory treats a molecule as a collection of nuclie with MOs delocalized over the entire structure(T,F)
T
The orbitals resulting from sp3d2 hybridization are directed toward the corners of an octahedron(T,F)
T
4 electron groups are____________, the possible molecular arrangements are___________________
Tetrahedral AX4, 109.5, Tetrahedral, Not flat AX3E1,, 107.5ish, trigonal pyramidal, not flat AX2E2, 105ish, Water bent
The principal quantam number(N) describes_______________, what is the N for copper
The level or shell of the orbital 3
Put brackets around a lewis structure when______________
There is a charge
5 electron groups are___________, the possible molecular arrangements are________________
Trigonal bipyramidal AX5, 90, 120, 180, Trigonal bipyramidal, not flat AX4E1, 90, 117, 180, seesaw, not flat AX3E2, 90, 80, T shaped panar, AX2E3, 190, Linear
3 electron groups are_________, the possible molecular arrangements are_____________
Trigonal planar, AX3, 120, trigonal planar AX2E1, 117, Bent(V-shaped)
The overlap of________ unhybridized orbitals oriented in the same way characterizes one ______, and _________ unhybridized orbitals results in two pi bonds
Two pi bond Four
When comparing lengths of bonds, first u compare _______________ then____________
Type of bond(single,double, triple) Size
En Trends
Typically down .5 right to left typicallly down by half on row 7
Pi bond overlaps side to side making it ________ than the overlapping sigma bond
Weaker
Lattice energy is the energy required _______________________________
When one more of an ionic solid separates into gas phase ions
The magnetic quantum number describes_________________________, what is the magnetic quantum number for Cu?
Which orbital the last electron can be in 2
Ga 3+ electron configuration
[Ar] 3d10(psuedo noble gas)
Cr3+ econfig
[Ar] 3d3
ln + Econfig
[Ar] 5s2 4d10
Condensed electron configuration for Sb
[Kr] 5s2 4d10 5p3
The ability for an element to attract electrons is known as_______________
electronegativity
Which of the following statements concerning polar molecules is false? 1.) molecule with symmetrically arranged polar bonds can be polar if the central atom is bonded to atoms of different elements. 2.) There must be an odd number of polar bonds so that their polarities not cancel. 3.) If there are more than one unshared pair of electrons on the central atom, they must not be symmetrically arranged so that their polarities cancel. 4.) There must be at least one polar bond or one unshared pair of electrons on the central atom. 5.) If there are more than one polar bond, they must not be symmetrically arranged so that their polarities cancel.
2, why?
Shape of P orbital
3 x dumbell
Which of the following statements cocncerning the benzene molecule, C6H6, is false 1.) The entire benzene molecule is planar. 2.) All six of the carbon-carbon bonds have the same length. 3.) Valence bond theory describes the molecule in terms of 3 resonance structures. 4.) The valence bond description involves sp2 hybridization at each carbon atom. 5.) The carbon-carbon bond lengths are intermediate between those for single and double bonds.
3, why?
How many Outer electrons in PB: [Xe] 6s2 5d10 4f14 6p2
4
Valance electrons in Ge: [Ar] 4s2 3d10 4p2 Fe?: 4s2 4d6
4 8
Shape of D orbital
4 x flower thing 1 x dumbell with circle round it
Which statement is false? 1.) In MO theory all electrons are accounted for, not just the valence electrons. 2.) Electrons occupy MOs by following the Aufbau Principle. 3.) Electrons occupy MOs by following Hund's Rule. 4.) Electrons occupy MOs by following the Pauli Exclusion Principle. 5.) No two molecular orbitals for any molecule ever have the same energy.
5
How many inner electrons does PB have? Ar?
78 18
What are all of the polar VESPER shapes(dipole moments)?
AX2E1(Bent, V-shaped) AX3E1(Trigonal pyramidal) AX2E2(Bent, water bent) AX4E1(Seesaw) AX3E2(T-shaped Planaar) AX5E1(Square pyramidal)
Two or more metals form metallic bonds which are_____________-
Alloys
More metallic Oxides form_____________ more nonmetal Oxides form__________
Bases, Acids