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52 Terms

1

Covalent Bond

A bond formed from atoms sharing electrons.

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2

Molecule

A covalent compound made up of two or more atoms.

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3

Formula Unit

The lowest whole number ratio of ions in an ionic compound.

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4

Octet Rule

Atoms become stable by having eight electrons in their valence shell.

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5

Diatomic Elements

Elements that naturally bond to themselves, like H2 or O2.

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6

Single Covalent Bond

A bond formed by the sharing of one pair of electrons.

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7

Double Covalent Bond

A bond formed by the sharing of two pairs of electrons.

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8

Triple Covalent Bond

A bond formed by the sharing of three pairs of electrons.

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9

Bond Length

The distance between the nuclei of two bonded atoms.

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10

Bond Dissociation Energy

The amount of energy required to break a specific covalent bond.

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11

Endothermic Process

A process that absorbs energy, such as breaking bonds.

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12

Covalent Compound Naming Rule

Use prefixes based on subscripts, change the ending of the second element to -ide.

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13

Hydro_ic Acid

Naming convention for binary acids that end in -ide.

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14

Monocyclic Hydrocarbons

Simple hydrocarbons with carbon and hydrogen only.

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15

Alkane Formula

CnH2n+2, where C is the number of carbon atoms.

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16

Alkene Formula

CnH2n, indicating double bonds present.

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17

Alkyne Formula

CnH2n-2, indicating triple bonds present.

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18

Unsaturated Hydrocarbons

Hydrocarbons with double or triple bonds.

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19

Saturated Hydrocarbons

Hydrocarbons that contain only single bonds.

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20

Cyclic Hydrocarbons

Hydrocarbons that form a ring structure.

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21

Alcohol Naming Rule

Drop the -ane from the alkane name and add -anol.

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22

Lewis Structure

Diagram showing the arrangement of valence electrons around atoms.

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23

Central Atom Rule

The least electronegative atom is generally the central atom.

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24

VSEPR Theory

Valence Shell Electron Pair Repulsion, predicts molecular shapes.

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25

Trigonal Planar Geometry

Molecular shape with 3 bonding pairs and 0 lone pairs.

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26

Tetrahedral Geometry

Molecular shape with 4 bonding pairs and 0 lone pairs.

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27

Resonance

Occurs when two or more valid Lewis structures can represent a molecule.

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28

Polar Covalent Bond

A bond where electrons are shared unequally due to electronegativity differences.

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29

Nonpolar Covalent Bond

A bond where electrons are shared equally.

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30

Ionic Bond

A bond formed by the complete transfer of electrons.

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31

Electronegativity

A measure of an atom's ability to attract and hold electrons.

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32

Intermolecular Forces

Forces that occur between molecules, which are generally weak.

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33

Hydrocarbons

Compounds made solely of hydrogen and carbon.

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34

Aromatic Compounds

Compounds that contain a benzene ring.

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35

Square Planar Geometry

Molecular shape with 4 bonding groups and 2 lone pairs.

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36

Seesaw Geometry

Molecular shape with 4 bonding groups and 1 lone pair.

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37

Straight-chain Hydrocarbons

Hydrocarbons with carbon atoms connected in a linear arrangement.

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38

Cyclic Alkanes

Cyclic hydrocarbons following specific bonding patterns.

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39

Bond Character Dependence

Determined by the electronegativity difference of bonded atoms.

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40

Alcohols in Chemistry

Compounds with a hydroxyl group (-OH) bonded to a carbon atom.

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41

Naming Binary Acids

Use the prefix 'hydro' for acids not containing oxygen.

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42

Forces in Covalent Compounds

Covalent bonds are strong, but intermolecular forces are weak.

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43

Shape Symmetry in Molecules

Symmetrical shapes tend to be nonpolar if terminal atoms are identical.

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44

Lowest Melting/Boiling Points

Covalent compounds usually have lower melting and boiling points due to weak intermolecular forces.

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45

Lone Pairs and Bonding

Unshared pairs of electrons impact molecular geometry and polarity.

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46

Hydrogen as a Central Atom

Hydrogen can never be the central atom in a Lewis structure.

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47

Diatomic Element Examples

H2, N2, O2, F2, Cl2, Br2, I2 are all diatomic elements.

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48

Shape Determinants

The geometry and symmetry of a molecule impact its polarity.

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49

Organic Compound Naming Rules

Name compounds starting with carbon and containing many hydrogens.

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50

Acid Naming Rule

Compounds starting with H follow specific acid naming rules.

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51

Electronegativity Difference Importance

Determines whether a bond is ionic, polar covalent, or nonpolar covalent.

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52

Bonding Energy Relation

Shorter bond lengths correspond to greater bond dissociation energy.

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