AP Chemistry Unit 2 Review

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Ionic bond

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37 Terms

1

Ionic bond

A bond between a metal and nonmetal in which the metal loses an electron and the nonmetals gains one.

Avg. EN: Medium (one high, one low)

Difference in EN: Large

<p>A bond between <strong>a metal and nonmetal</strong> in which the metal loses an electron and the nonmetals gains one.</p><p><strong>Avg. EN:</strong> Medium (one high, one low)</p><p><strong>Difference in EN:</strong> Large</p>
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2

Covalent/Molecular Bond

A bond between nonmetals in which atoms share electrons to fill their valence shells; they all “grab” electrons

Avg. EN: High

Difference in EN: Small (lower if nonpolar, medium if polar)

<p>A bond between <strong>nonmetals</strong> in which atoms share electrons to fill their valence shells; they all “grab” electrons</p><p><strong>Avg. EN:</strong> High</p><p><strong>Difference in EN:</strong> Small (lower if nonpolar, medium if polar)</p><p></p>
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3

Metallic bonds

A bond between metals in which metallic cations (positive ions) are attracted to a sea of electrons

Avg. EN: Low (metals want to lose electrons)

Difference in EN: Small

<p>A bond between <strong>metals</strong> in which metallic cations (positive ions) are attracted to a sea of electrons</p><p><strong>Avg. EN: </strong>Low (metals want to lose electrons)</p><p><strong>Difference in EN:</strong> Small</p>
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4

Electronegativity

A quantitative value used to measure the ability/desire of an atom to attract electrons to itself

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5

Bond Polarity

Polar = electrons are shared unequally.

The more unequal the EN, the more polar a bond is.

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Dipole Moment

The bigger the dipole moment, the more polar a bond is.

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Intramolecular Forces

There are two main forces within a molecule:

  1. 2 nuclei repel each other, 2 electrons repel each other

  2. Nuclei + electrons attract each other

<p>There are two main forces within a molecule:</p><ol><li><p>2 nuclei repel each other, 2 electrons repel each other</p></li><li><p>Nuclei + electrons attract each other</p></li></ol><p></p>
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Bond Types

Single: 1 pair (2 electrons)

Double: 2 pairs (4 electrons)

Triple: 3 pairs (6 electrons)

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Potential Energy

When there is little distance between atoms, there is a strong force of repulsion between the two, pushing them apart. When they reach a certain distance, called a “goldilocks zone,” there is a perfect amount of attraction between them. If they go too far apart, however, there will be no more attraction or repulsion between them.

<p>When there is little distance between atoms, there is a strong force of repulsion between the two, pushing them apart. When they reach a certain distance, called a “goldilocks zone,” there is a perfect amount of attraction between them. If they go too far apart, however, there will be no more attraction or repulsion between them.</p>
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10

Enthalpy

The average change in energy when a bond is broken- calculated by subtracting the total bond energy of the resulting bond from the energy from the starting bonds.

<p>The <em>average</em> change in energy when a bond is broken- calculated by subtracting the total bond energy of the resulting bond from the energy from the starting bonds.</p>
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Lattice Energy

The energy required to separate 1 mol of solids into gaseous ions (similar to enthalpy, but for lattices)

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Factors that determine Lattice Energy

(In order)

  1. Ion Charge: More positive/negative = stronger attraction = more lattice energy

  2. Ion Radius (size): Smaller = fewer energy levels = stronger Coulombic attraction = more lattice energy

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Higher lattice energy means…

…harder, higher melting point, less soluble (prone to being dissolved) in water

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Electron Removed From Metal

Ionization Energy

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Electron Added to Nonmetal

Electron Affinity/Electronegativity

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Ions Attract Each Other & Form Lattice

Opposite of lattice energy

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Metal Characteristics

Easily molded, electrically conductive

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Alloy

A material that contains multiple elements and has the characteristic properties of metals (examples: stainless steel, brass, etc.)

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Substitution Alloy

The solute (what’s being dissolved) takes positions normally occupied by a solvent (what causes the dissolving)

<p>The solute (what’s being dissolved) takes positions normally occupied by a solvent (what causes the dissolving)</p>
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Interstitial Alloy

Solute (what’s being dissolved) takes position in the holes between solvent (what causes the dissolving) atoms

<p>Solute (what’s being dissolved) takes position in the holes between solvent (what causes the dissolving) atoms</p>
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Resonance

Structures with different electron arrangements

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Isomers

Structures with different atom arrangements

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Formal Charge

The original number of valence electrons subtracted by the amount of unbonded electrons subtracted by half of the shared electrons

<p>The <strong><em>original</em></strong> number of valence electrons subtracted by the amount of unbonded electrons subtracted by <strong><em>half</em></strong> of the shared electrons</p>
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24

Dominant Structure

When formal charges are closest to zero OR when negative formal charge is on a more electronegative atom

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Traits of Delocalized Double Bonds

  1. Extra stability

  2. Between single bond & double bond in terms of length and strength

  3. The more places delocalized, the closer it is to a single bond

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Electron Domain

A group of electrons doing one “thing-” bonding or a lone pair

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Electron Geometry

The 3D spatial arrangement of electron pairs around a central atom so that they are as far away from each other as possible.

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Molecular Geometry

The three-dimensional arrangement of atoms in a molecule.

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2 domains

Name: Linear

Angle measure: 180Âş

Hybridization: sp

<p><strong>Name: </strong>Linear</p><p><strong>Angle measure: </strong>180Âş</p><p><strong>Hybridization: </strong>sp</p>
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3 domains

Name: Trigonal Planar

Angle measure: 120Âş

Hybridization: sp2

<p><strong>Name: </strong>Trigonal Planar</p><p><strong>Angle measure: </strong>120Âş</p><p><strong>Hybridization: </strong>sp<sup>2</sup></p>
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4 domains

Name: Tetrahedron

Angle measure: 109.5Âş

Hybridization: sp3

<p><strong>Name: </strong>Tetrahedron</p><p><strong>Angle measure: </strong>109.5Âş</p><p><strong>Hybridization: </strong>sp<sup>3</sup></p>
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5 domains

Name: Trigonal Bipyramid

Angle measure: 90Âş AND 120Âş

Hybridization: sp3d

<p><strong>Name: </strong>Trigonal Bipyramid</p><p><strong>Angle measure: </strong>90Âş <em>AND</em> 120Âş</p><p><strong>Hybridization: </strong>sp<sup>3</sup>d</p>
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6 domains

Name: Octahedron

Angle measure: 90Âş

Hybridization: sp3d2

<p><strong>Name: </strong>Octahedron</p><p><strong>Angle measure: </strong>90Âş</p><p><strong>Hybridization: </strong>sp<sup>3</sup>d<sup>2</sup></p>
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34

Traits of Polar Molecules

  • Some bonds must be polar

  • Its shape must be assymetrical

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35

Sigma Bonds

Literally ANY bond. All bonds are sigma

<p>Literally ANY bond. All bonds are sigma</p>
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36

Sigma Pi Bonds

Double Bonds

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Sigma Pi Pi Bonds

Triple Bonds

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