Chapter 8- Chemical Bonding

Question 1

Ionic

Answer 1

Metals and nonmetals

Unfair sharing of electrons

Question 2

Covalent

Answer 2

Nonmetals and nonmetals
Fair sharing of electrons
Can be polar or nonpolar

Question 3

Metallic

Answer 3

E cloud bonds atoms

Question 4

Octet rule

Answer 4

Atoms tend to lose or gain until they are surrounded by 8 electrons except H which needs two

Question 5

Polar bonds

Answer 5

Covalent bonds in which electrons are shared unequally die to the differences in the elements electronegativities

Question 6

Polar molecule (dipole)

Answer 6

A molecule containing a polar bond which results in an uneven distribution of electrons

Question 7

Dipole moment

Answer 7

Measurement of the magnitude of dipole

Question 8

Reasonable structures

Answer 8

Molecules with more than one plausible structure

Question 9

Lattice energy (Eel)

Answer 9

Energy required to completely separate 1 mol of an ionic crystal into its gaseous ions

Question 10

All ionic compounds

Answer 10

Are solid and exist as a crystal lattice

Question 11

Ionic bonds are ______ than covalent bonds

Answer 11

Stronger

Question 12

Formula for lattice energy

Answer 12

Eel = (constant times charges of ions) / distance between nuclei

Question 13

Lattice energy

Answer 13

All about charge and attraction

Question 14

Formal charge

Answer 14

The charge that an atom in a molecule would have if all of its bonding electron pairs were shared equally between atoms
(Allows us to predict correct form of a molecule)

Question 15

Formal charge adds up to

Answer 15

The charge of the ion

Question 16

Halogens only form

Answer 16

Single bonds

Question 17

Anything form the throw period down can

Answer 17

Hybridize

Question 18

Heat of reaction

Answer 18

Bonds broken-bonds formed

Question 19

VSEPR

Answer 19

Valance shell electron pair repulsion theory

Question 20

Electron pairs on a central atom

Answer 20

Bonded or unbounded will repel, thus creating the molecules shape

Question 21

Electron domains

Answer 21

The areas where the electrons are likely to be located

Question 22

Electron domain geometry

Answer 22

Shape created by the electron domains

Question 23

Molecular geometry

Answer 23

The shape created by the arrangement of atoms

Question 24

Shape of two electron domains

Answer 24

Linear (180 degrees)

Question 25

Shape of three electron domains

Answer 25

``` Trigonal planar (120) Bent(120) (one unbounded pair) ```

Question 26

Shape of four electron domains

Answer 26

``` Tetra hedral (109) Trigonal pyramidal (107) Bent (two unbounded electrons) (104) ```

Question 27

Tetrahedral

Answer 27

109

Question 28

Trigonal pyramidal

Answer 28

107

Question 29

Bent (one unbounded electron pair)

Answer 29

120

Question 30

Bent (two unbounded electron pairs)

Answer 30

104

Question 31

Trifocals planar

Answer 31

120

Question 32

How does a bond affect a molecules polarity

Answer 32

A polar bond "bond dipole" is a vector quantity. Therefore it has magnitude and direction

Question 33

Bonding site

Answer 33

Orbital with only one electron in it

Question 34

Valance bond theory

Answer 34

Covalent bonds are formed by overlapping atomic orbitals which contain electrons

Question 35

Does orbital overlap happen in polyatomic molecules?

Answer 35

Yes but the atomic orbitals (s,p,d) mix to form a hybrid orbital

Question 36

Linear

Answer 36

Sp

Question 37

Trifocals planar

Answer 37

Sp2

Question 38

Tetrahedral

Answer 38

Sp3

Question 39

Covalent bonds can be classified as

Answer 39

Sigma or pi bonds

Question 40

Sigma bond

Answer 40

End to end overlap of atomic orbitals

Question 41

The electron density of sigma bonds

Answer 41

Is concentrated along a line that connects the nuclei

Question 42

Pi bond

Answer 42

A side by side overlap of Unhybridized atomic orbitals

Question 43

Electron density of pi bonds

Answer 43

Is concentrated above and below a line that connects the nuclei

Question 44

Single bond

Answer 44

Sigma bond

Question 45

Double bond

Answer 45

One sigma | One pi

Question 46

Triple bond

Answer 46

One sigma | Two pis

Question 47

Electronic geometry may be different from molecular geometry because

Answer 47

The electronic geometry refers to how the electrons are arranged, but the molecular geometry indicates the net shows of the molcule

Question 48

VSEPR theory is based on

Answer 48

Minimization of repulsion among valance electron pairs

Question 49

The central atom in compounds with square planar geometric always abet the octet rule

Answer 49

True

Question 50

Large electronegativities difference affects molecular properties

Answer 50

By making boss stronger and shorter Makes bonds highly polar Makes molecule highly polar if molecular geometry permits

Question 51

Metallic bond

Answer 51

Metals and metals | Electron clouds around atom