AP Chem Unit 3 Study Guide

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THINGS TO REVIEW: -Dot Diagrams -Shape -Bond Angles -Polarity -Counting sigma bonds

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31 Terms

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What is Ionic Bonding

  • The transfer of electrons

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What is a lattice and what is lattice energy?

Lattice = stable, ordered, solid 3D array of ions

Lattice Energy = The energy required to completely separate a mole of a solid ionic compound into gaseous ions

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Use Coulombs law to justify lattice energy

Greater charge = greater charge (increases across)

Greater distance = weaker attraction (decreases down)

  • always look at charge first (greater the charge greater the lattice energy)

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Characteristics of Ionic Solids (6 characteristics)

  • Hard

  • Brittle

  • High Melting Points

  • Transition Metals loses e-

  • Mostly soluble in water

  • Does NOT conduct as a solid

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What is a amorphous solid?

A solid where the arrangement lacks any pattern

  • ex) glass, wax, and sand

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Ionic Solids (3 Parts: Formula, Structure/Bonding, Properties

Recognizing a Formula

  • Compounds of metal cations + nonmetal anions. ex) NaCl FeS

Structure & Bonding

  • 3D locked in place by strong ionic bonds

Properties

  • Brittle

  • High Melting

  • Non-conductors in water

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Metallic Solid

Recognizing a Formula

  • Metal atoms ONLY

Structure & Bonding

  • 3D metal ions surrounded by delocalized e- (do not belong to any atom/they move freely about the network)

Properties

  • Good conductors of heat & electricity

  • Malleable

  • Ductile

  • Alloys

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Covalent-network solids

Recognizing a Formula

  • Carbon (graphite & diamond); metalloids: Si, Ge; and compounds of metalloids (SiC, BN)

Structure & Bonding

  • An extended network of covalent bonds

Properties

  • Hard

  • High-Melting

  • Insoluble in water

  • Doesn´t conduct heat or electricity

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Molecular solids

Recognizing a Formula

  • Compounds of nonmetals ONLY

Structure & Bonding

  • Individual contently bonded molecules held together by weak inter molecular forces

Properties

  • Soft

  • Low-Melting

  • Nonconductors

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How do metallic bonds form?

Outer energy levels overlap

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Subsitutional Alloys

A homogeneous alloy in which different atoms of similar size occupy sites in the lattice

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Interstitial Alloys

Where smaller atoms (usually nonmetals) fit into spaces between larger atoms (usually a metal)

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Covalent Bonding

Sharing of e-

  • Low-Melting

  • Don´t dissolve easily in water

  • Doesn´t conduct electricity in solutions

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Electronegativity Difference and how that determines the type on bonds

0-0.4 = Nonpolar covalent

0.4-2.0 = Polar covalent

> 2.0 = Ionic

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Polar Covalent Bond

  • unequal sharing of electrons

  • dipole moment

    • A dipole moment is a measurement of the separation of two opposite electrical charges (magnitude x distance = charge)

    • A measurement of 2 electrical charges creates a dipole moment

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Nonpolar Covalent Bond & Shapes that are ALWAYS Nonpolar

equal sharing of electrons

  • Linear

  • Trigonal Planar

  • Tetrahedral

  • Square Planar

  • Octahedral

  • Trigonal Bipyramidal

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Exceptions to Lewis Dot Structures

  • H only needs 2 e-

  • Groups 1, 2, 13 need twice their # of e-

  • O & F can’t be the central atom

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What is resonance

Multiple ways of drawing the same structure

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How to determine the best structure

  1. Count e- in line pairs and ½ e- it shares for each atom

  2. Subtract from the # of e- for that atom

  • Best structure = one with the fewest charge

  • Puts a negative charge on the most EN atom

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What does VESPER theory describe?

The repulsion between electron pairs causes molecular shapes to adjust so that the valence-electron pairs stay as far away as possible.

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VESPER Theory : Nonbonding/Lone Pairs

Subtract 2 for every lone pair from the original angle

  • repulsion →smaller angle

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VESPER Theory: Multiple(triple or double) Bonds affect bond angles

Place greater e- density on 1 side of the central atom than do single bonds

  • expands angle → >120 degrees

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How to analyze larger molecules (refer back to page 8 of note packet)

  • Look at 1 particle atom instead of the molecule as a whole

  • Split it

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Sigma Bond

  • head-head overlap: cylindrical

  • symmetry of e- density about the inter-nuclear axis

  • ALL SINGLE BONDS

  • STRONGER than pi bonds

SINGLE BOND = 1 SIGMA (the 6 looking symbol)

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Pi Bonds

  • side-side overlap

  • e- density below inter-nuclear axis

  • founding double and triple bonds

Delocalized pi bonding

  1. resonance

  2. double/triple bonds

Double Bond —> 1 6 + 1π

Triple Bond —> 1 6 + 2π

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How to read inter-nuclear distance graphs

  • bond length = distance between atoms goes across

  • bond energy does up & down

the greater the charge the stronger the bond energy and the shorter the bond length

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Linear

Bonded: 2

Lone: 0

Angle: 180

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Trigonal Planar

Bonded: 3

Lone: 0

Angle: 120

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Tetrahedral

Bonded: 4

Lone: 0

Angle: 109.5

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Trigonal Bipyramidal

Bonded: 5

Lone: 0

Angle: 90 & 120

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Octahedral

Bonded: 6

Lone: 0

Angle: 90