Chemistry Exam 3 Memorization

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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


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