1B Chemical Bond Flashcards by Brittany Lazenby

Effects of metallic bond

Isotropic bond/force causes equal atomic sizes causes simple packing

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Packing form of 80% all metallic elements

HCP, FCC, BCC

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HCP packing

ABABABABABAB…

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FCC/CCP Packing

ABCABCABCABC

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Different types of strong chemical bonds

Metallic, ionic, covalent

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Weak chemical bonds

Hydrogen bonds, van der waals interactions (London, Debye, keesom)

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Pure elements and alloys

Metals

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Characteristics of metals

Few electrons in valence shell; low atomic ionization energies (<10 eV); not transparent, metal,ice shine, ductile, good conductor; wide range of melting points

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Relationship btwn electric conductivity and temp for metals

Decreases as temp increases

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Relationship btwn electric conductivity and temp for metalloids

Increases as temp increases

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Metallic bonds form between … bc…

Similar metals because similar radii leads to simple packing patterns. And the metal character

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Zintl phases form between

Metals with high ΔEN (s-p) because the bond character between metallic and ionic. Has metal kind character. Often polyatomic Anions with covalent scaffold

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Ionic bonds form between

Metal nonmetal compounds with ΔEN > 1.5. Large nonmetal anion with small, metal cation allows complex packing. Salt character

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Differences between metals: main group

S and P valence orbitals, fewer oxidation states

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Differences between metals: transition metals

S and D valence orbitals have more oxidation states

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Main group metal ions description

Noble gas config. Diamagnetic, colorless, not precious

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Transition metal ion descriptions

Can possess partially filled d orbitals. Potentially colorful and paramagnetic and can be precious

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Metallic Bond by Drude and Lorentz

Delocalized valence electron cloud around atomic cores

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Metallic Bond by Drude and Lorentz characteristics

Isotropic bond/force causes equal atomic sizes leading to simple packing

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Ductility of the packing from softest to hardest

FCC > HCP > BCC

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Effect on hardness by the transition from heteroatoms to alloys

Increases hardness

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Packing between condensed noble gases?

Similar to metal packing bc of isotropic London forces between equal atoms

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What causes ductility

Layered structure

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Direct packing

Band energies (electronics)

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Can drude lorentz theory predict packing type

Nope

HCP

Hexagonal close packed

Common HCP elements

Zinc, magnesium, cadmium

FCC or CCP

Face centered aka cubic close. Think of a dice

Common FCC/CCP elements

Aluminum, copper, silver

BCC

Body centered cubic. Think of it floating in the middle of a box

Common BCC elements

Chromium, tungsten, iron

Mixing similar metals gives you

Alloys

Mixing very different metals gives you

Zintls

How to calculate ionic band

Coulomb force

Inionic Lattice vs metallic

Similar

What does it mean that Coulomb force is isotropic

Works in all directions

How many atoms are around?

Coordination number

Void for Cord 2

Linear

Void for cord 3

Triangular planar

Void for cord 4

Tetrahedral

Void for cord 6

Octahedral

Void for cord 8

Cubic

Void for cord 12

Close packing CCP and HCP. In metals

Lattice energy is true for

Isolated pairs

Madelung constant is lattice dependent or independent?

Lattice dependent

Lattice energy effect on dissolving

High lattice energy means harder to dissolve. Can heat to help

Higher Lattice energy effect on melting point

Higher melting point

3 types of point defects

Vacancy, interstitial, substitution

Needed to create defects?

Energy

Vacancy by moving to interstitial site

Frenkel type defect

Vacancy by moving to crystal surface

Schottky type defect

Intrinsic lattice defect

Pure compound

Extrinsic lattice defect

Additional of dopant

What happens if you add a dopant with additional valence electrons

Changes the color!

Nonpolar covalent bond ΔEN

ΔEN < 0.5 or 0.7

Polar covalent ΔEN

0.5 or 0.7 < ΔEN < 1.5 or 1.7

Ionic ΔEN

ΔEN > 1.5 or 1.7

Equal shading of valence electrons

Nonpolar covalent

Unequal sharing of valence electrons

Polar covalent

Valence Bond theory based on

Orbital theory application of schrodingers wave equation

Valence bond theory explains covalent bonding as

Overlap of atomic orbitals

Orbitals according to VB theory

Still localized on atoms

Interactions between 2 isolated H atoms with Ha e1 and Hb e2?

Core A + e1 and Core B + e2

Interactions between 2 hydrogen atoms that approach each other

Core A + e1 Core B + e2 Core A + e2 Core B + e1 e1 + e2 Core A + Core B

Total energy when no interaction between 2 hydrogen atoms

E total = EA + EB

Total energy between 2 hydrogen atoms approaching each other

E total DOES NOT EQUAL Ea + Eb

Heisenberg's Uncertainty Principle

Electrons of close atoms cannot be differentiated. Electron 1 and e2 can both be assigned to either Ha or Hb

ψ+ represents

Spin coupled state

Does ψ+ obey Pauli?

Yeah

ψ+ stable or unstable

Stable

ψ- represents

State with parallel spins

ψ- stability

Unstable

Electrons in ψ+ or ψ- have more space?

ψ+ so they can get closer to cores

Electrons that can get closer to cores leads to what kind of electron density

High

The bond is located in the

Density between cores

Constructive interference of different atomic orbitals

Attractive

Destructive interference of different atomic orbitals

Repulsive

Non constructive interference of different atomic orbitals

No interactions

Can the original valence bond theory predict geometry

No it cannot

Hybridization of atomic orbitals based on

Orbital theory. Application of schrodingers wave equatjon

Hybridization of atomic orbitals is an expansion of

Valence bond theory

Explain hybridization of atomic orbitals

Linear combo of atomic orbitals (LCAO) Only AOs of the same atom are combined /hybridized

x AOs in hybridization of AO theory become

x hybrid AOs

percent s character in sp3

25%

Percent s character in sp2

33%

orbital geometry in sp

Linear. 180°

Orbital geometry of sp2

Triangular planar 120°

Orbital geometry of sp3

Tetrahedral 109.5°

Orbital geometry of sp3d

Trigonal bipyramidal 90° and 120°

Orbital geometry of sp3d2

Octahedral 90°

MO theory orbitals and electrons placement

Orbitals/electrons spread over whole molecule! Not localized at single atoms

Lewis form in MO

Not compatible

MO theory AOs combination

AOs of all atoms in same molecule or ion are combined

In MO theory, x AOs =

x MOs

AOs symbolized with

Roman letters like s p d

ΜOs are symbolized with

Greek letters like σ π δ

Antibonding MOs marked by

An asterisk like σ*

Bond order equation

BO = (#e in binding MO) - (#e in antibinding MO) divided all by 2

Hybrids symmetry

Hybrids are asymmetric

MO binding electrons

Not assigned to individual bonds between atoms

VB theory explains covalent bonds as

Overlap of atomic orbitals

VB Orbitals

Localized on atoms

difference between main group and transition metals oxidation states

transition metals have more oxidation states

smaller Madelung Constant (A) means

not good packing

Which has a node? Spin couple or parallel spins?

parallel

hybridization of linear

hybridization of triangular planar

sp2

hybridization of tetrahedral

sp3

hybridization of trigonal bipyrimidal

sp3d

hybridization of octahedral

sp3d2

destructive overlap can cause a

nodal plane

What needs more space? single bond, double bond, or lone pair?

lone > double > single

metal + metal =

metallic bond

metal + nonmetal =

ionic bond

nonmetal + nonmetal =

covalent bond

metalloid + metal =

metallic bond

metalloid + nonmetal =

covalent bond

1B Chemical Bond Flashcards

(117 cards)