Words Flashcards

1
Q

A neutral group of atoms joined together by covalent bonds

A

Molecule

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2
Q

A molecule that contains 2 atoms

A

Diatomic molecule

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3
Q

A compound composed of molecules

A

Molecular compounds

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4
Q

The chemical formula of a molecular compound

A

Molecular Formula

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5
Q

Two atoms held together by sharing one pair of electrons are joined by a…

A

Single Covalent Bond

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6
Q

Represents the covalent bonds as dashes and shows the arrange,ent of covalently bonded atoms

A

Structural Formula

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7
Q

A pair of valence electrons that is not shared between atoms

A

Unshared Pair

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8
Q

A bond that involves two shared pairs of electrons

A

Double Covalent Bond

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9
Q

A bond formed by sharing three pairs of electrons.

A

Triple Covalent Bond

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10
Q

A covalent bond in which one atom contributes bith bonding electrons

A

Coordinate Covalent Bond

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11
Q

A tightly bond group of atoms that has a positive or negative charge and functions as a unit

A

Polyatomic Ion

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12
Q

The energy required to break the bond between two covalently bonded atoms

A

Bond Disassociation Energy

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13
Q

Structures that occur when it is possible to draw two or more valid electron dot structures that have the same amount of electron pairs for a molecule or ion.

A

Resonance Structures

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14
Q

Orbitals that apply to the entire molecule

A

Molecular Orbitals

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15
Q

A molecular orbital that can be occupied by two electrons of a covalent bond

A

Bonding Orbital

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16
Q

When two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting two atomic nuclei, a _____
is formed. The orbitals in this type of bond overlap end to end.

A

Sigma Bond

17
Q

In some molecules, orbitals can overlap side-by-side. The side-by-side overlap of atomic p orbitals produces what are called ____ molecular orbitals. When a ____ molecular orbital is filled with two electrons, a ____ bond results. In this bond, the bonding electrons are most likely to be found in two sausage-shaped orbitals above and below the bond axis of atoms; weaker than sigma bond.

A

Pi Bond

18
Q

In this molecular arrangement, all the bond angles are 109.5*. Four corners of a regular geometric solid.

A

Tetrahedral Angle

19
Q

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

A

VSEPR Theory

20
Q

In this process, several atomic orbitals mix to form the same total number of equivalent hybrid orbitals

A

Hybridization

21
Q

When the atoms in a covalent bond pull equally (as occurs when identical atoms are bonded), the bonding electrons are shared equally, and each bond formed is a ________.

A

Nonpolar Covalent Bond

22
Q

A covalent bond between atoms in which the electrons are shared unequally.

A

Polar Covalent Bond/ Polar Bond

23
Q

A molecule that has two poles

A

Dipolar molecule (dipole)

24
Q

The two weakest intermolecular attractions—dispersion interactions and dipole forces.

A

Van der Waals Forces

25
Q

Intermolecular forces resulting from the attraction of oppositely charged regions of a polar molecule.

A

Dipole Interactions

26
Q

Attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules.

A

Dispersion forces

27
Q

Attractive forces in which a hydrogen covalently bonded to a very electronegative atom is also weakly bonded to an unshared pair of another electronegative atom.

A

Hydrogen Bonds

28
Q

A solid in which all of the atoms are covalently bonded to each other.

A

Network Solid

29
Q

Atoms that are held together by sharing electrons are joined by a…

A

Covalent Bond