Chemistry Test 4 Chapter 10B

Front 1

Two atoms on opposite sides of central atom.
180° bond angles.

Back 1

Linear
Geometric Figures

Front 2

Three atoms form a triangle around the central atom.
Planar.
120° bond angles.

Back 2

Trigonal planar
Geometric Figures

Front 3

Four surrounding atoms form a tetrahedron around the central atom.
109.5° bond angles.

Back 3

Tetrahedral
Geometric Figures

Front 4

In ____ ____ molecules are three-dimensional objects.

Back 4

Molecular Geometry

Front 5

In ___ ___ we often describe the shape of a molecule with terms that relate to geometric figures.

Back 5

Molecular Geometry

Front 6

In ___ ___ the geometric figures have characteristic “corners” that indicate the positions of the surrounding atoms with the central atom in the center of the figure.

Back 6

Molecular Geometry

Front 7

The geometric figures also have characteristic angles that we call _____________.

Back 7

bond angles.

Front 8

Negatively-charged electron groups around the central atom will be most stable when they are as far apart as possible. We call this __ __ __ __ __ __ ( ___ )

Back 8

valence shell electron pair repulsion theory (VSEPR).

Front 9

“Electron groups” include:

Back 9

Single bonds
Double bonds
Triple bonds
Lone pairs

Front 10

The Lewis structure predicts the arrangement of ___ ___ around the ______ atom(s).

Back 10

valence electrons, central

Front 11

Each lone pair of electrons constitutes __ ___ __on a central atom.

Back 11

one electron group

Front 12

Each bond constitutes one electron group on a ____ ___.
Regardless of whether it is single, double, or triple.

Back 12

central atom

Front 13

Balloons behave like _____ ___! Will align themselves to be as far apart as possible.

Back 13

electron-groups

Front 14

When ___ a ___ because molecules are three-dimensional objects, our drawings should indicate their three-dimensional quality

Back 14

Sketching, Molecule

Front 15

By convention:
A ______ wedge indicates that the attached atom is coming out of the paper toward you.
A ______ wedge indicates that the attached atom is going behind the paper away from you.

Back 15

filled, dashed

Front 16

__-___ ___ describes the arrangement of electron groups around a C.A.

Back 16

Electron-pair geometry

Front 17

______ ___ describes the arrangement of atoms around a C.A.

Back 17

Molecular geometry

Front 18

If all electron-groups around C.A. are bonding groups: __ __ __ = __ ___

Back 18

electron-pair geometry = molecular geometry

Front 19

If there are lone-pairs on the C.A.: __ __ __ Does not equal __ __ __

Back 19

electron-pair geometry ≠ molecular geometry

Front 20

Electron groups on central atom = 2.
Bonding groups = 2.
Lone pairs = 0.

Back 20

Molecular Geometry: Linear

Front 21

Electron pair AND molecular geometry = linear.

Back 21

Molecular Geometry: Linear

Front 22

Bond Angle = 180°.

Back 22

Molecular Geometry: Linear

Front 23

Electron groups around central atom = 3.
Bonding groups = 3.
Lone pairs = 0.

Back 23

Molecular Geometry: Trigonal Planar

Front 24

Electron pair AND molecular geometry = trigonal planar.

Back 24

Molecular Geometry: Trigonal Planar

Front 25

Bond Angle = 120°.

Back 25

Molecular Geometry: Trigonal Planar

Front 26

Electron groups around central atom = 4.
Bonding groups = 4.
Lone pairs = 0.

Back 26

Molecular Geometry: Tetrahedral

Front 27

Electron-pair geometry AND Molecular geometry = tetrahedral.

Back 27

Molecular Geometry: Tetrahedral

Front 28

Bond Angle = 109.5°.

Back 28

Molecular Geometry: Tetrahedral

Front 29

Use Lewis Structure to determine if there are lone-pairs on __.

Back 29

C.A.

Front 30

___ __ on ___ repel other electron groups.
-Actually occupy more space than a bonding-pair.

Back 30

Lone-pairs on C.A.

Front 31

__ __ __ is relevant to Molecular geometry.
-Lone-pair(s) exert(s) influence on bonding-groups.

Back 31

Electron-pair geometry

Front 32

Electron groups around central atom = 3.
Bonding groups = 2.
Lone pairs = 1.

Back 32

Molecular Geometry: Bent

Front 33

Electron geometry = trigonal planar.

Back 33

Molecular Geometry: Bent

Front 34

Molecular geometry = bent

Back 34

Molecular Geometry: Bent

Front 35

Bond angle = < 120°.

Back 35

Molecular Geometry: Bent

Front 36

4 electron groups on the central atom:
Electron-pair geometry is ____________

Back 36

Tetrahedral

Front 37

If none of those groups is a lone pair:
Molecular Geometry is ____________
Bond angle: 109.5

Back 37

Tetrahedral

Front 38

If one of those groups is a lone pair:
Molecular Geometry is ______ _____
Bond Angle: < 109.5 

Back 38

Trigonal Pyramidal.

Front 39

If two are lone pairs:
Molecular Geometry is ______ (____)
Bond Angle: < 109.5 

Back 39

Bent (Angular)

Front 40

4 electron groups:
3 bonding pairs, 1 lone-pair

Back 40

Trigonal Pyramid

Front 41

4 electron groups:
2 bonding-pairs, 2 lone-pairs

Back 41

Bent (Angular)

Front 42

Electron groups around central atom = 4.
Bonding groups = 2.
Lone pairs = 2.

Back 42

Molecular Geometry: Bent

Front 43

Electron groups around central atom = 4.
Bonding groups = 2.
Lone pairs = 2.
Electron geometry = tetrahedral.

Back 43

Molecular Geometry: Bent

Front 44

Electron groups around central atom = 4.
Bonding groups = 2.
Lone pairs = 2.
Bond Angle < 109.5°.

Back 44

Molecular Geometry: Bent

Front 45

Bonding between unlike atoms results in unequal sharing of the electrons.
One atom pulls the electrons in the bond closer to its side.
One end of the bond has larger electron density than the other.

Back 45

Bond Polarity

Front 46

In Bond Polarity
The end with the larger electron density gets a ____ ___ __ and the end that is electron deficient gets a ___ ___ ___; a Dipole (not formal charges)

Back 46

partial negative charge, partial positive charge

Front 47

The ability of an atom to attract electrons to itself.

Back 47

Electronegativity

Front 48

Increases across the period (left to right).

Back 48

Electronegativity

Front 49

Decreases down the group (top to bottom).

Back 49

Electronegativity

Front 50

The larger the difference in ____________, the more polar the bond.
-Negative end toward more _________ atom.

Back 50

Electronegativity, electronegative

Front 51

If the difference in electronegativity between bonded atoms is 0 to 0.3, the bond is ________.

Back 51

pure covalent (non-polar)

Front 52

If the difference in electronegativity between bonded atoms is 0.4 to 1.9, the bond is _________.

Back 52

polar covalent

Front 53

If the difference in electronegativity between bonded atoms larger than or equal to 2.0, the bond is _______.

Back 53

ionic

Front 54

In order for a molecule to be polar it must have ____ ___ and an ______ ____.

Back 54

polar bonds, an unsymmetrical shape

Front 55

_____ effects the intermolecular forces of attraction (future chapter)

Back 55

Polarity

Front 56

The O—C bond is polar. The bonding electrons are pulled equally toward both O ends of the molecule (cancel each other out).

The net result is a _________

Back 56

non-polar molecule

Front 57

The H—O bond is polar.

Both sets of bonding electrons are pulled toward the O end of the molecule (do not cancel each other out).

The net result is a ________.

Back 57

polar molecule

Front 58

“If all atoms bonded to the central atom are identical, and there are no lone-pairs on the central atom, the molecule is non-polar. In all other cases, the molecule is polar”.

Back 58

Polarity Statement

Front 59

“If all atoms bonded to the central atom are identical, and there are no lone-pairs on the central atom, the molecule is ________. In all other cases, the molecule is _______”.

Back 59

non-polar, polar

Front 60

“If all atoms bonded to the central atom are identical, and there are no lone-pairs on the central atom, the ________ is non-polar. In all other cases, the _______ is polar”.

Back 60

molecule, molecule