Chemical Bonding

Question 1

alloy

Answer 1

A mixture of metals that acts like a metallic bond

Question 2

anion

Answer 2

negatively charged particle

Question 3

cation

Answer 3

positively charged particle

Question 4

chemical bond

Answer 4

a force that holds atoms together in a compound

Question 5

conductivity

Answer 5

The ability to allow heat or electricity to pass through an object

Question 6

covalent bond

Answer 6

A chemical bond created by the sharing of electrons

Question 7

ductility

Answer 7

the ability to be drawn into a wire

Question 8

Elctronegatjvity

Answer 8

an atoms ability to attract electrons

Question 9

ion

Answer 9

a charged particle

Question 10

ionic bond

Answer 10

a chemical bond created by the attraction between cations and anions whew electrons are exchanged

Question 11

luster

Answer 11

shininess

Question 12

malleability

Answer 12

ability to change shape without breaking

Question 13

metallic bond

Answer 13

a chemical bond formed when the sea of de localized electrons flows between metal atoms

Question 14

oxidation number

Answer 14

the charge an Tom has when it becomes an ion

Question 15

polar covalent bond

Answer 15

a covalent bond where electrons are not shared equally

Question 16

Polyatomic ion

Answer 16

an ion contacting multiple atoms covalent,y bonded

Question 17

salt

Answer 17

common name for ionic compounds

Question 18

Lewis dot structure

Answer 18

Diagrams showing the number of paired and unpaired electrons in a compound

Question 19

VSEPR model

Answer 19

Valence Shell Electron Pair Repulsion Model

Question 20

Compare and contrast ionic, covalent, and metallic bonding

Answer 20

Ionic-transferring electrons
Covalent-sharing electrons
Metallic-bonding with the “sea” of electrons

Question 21

How can you tell from a chemical formula if a compound is ionic or covalent

Answer 21

Ionic- metal and non metal

Covalent- two or more nonmetal

Question 22

List the proper iTunes of an ionic compound (salts) and describe how they form:

Answer 22

They form by transferring electrons
They have strong bonds
Crystalline structure
High melting points
Brittle
Conduct electricity in solution

Question 23

List the properties of covalent compounds (molecules) and describe how they form

Answer 23

They form from sharing electrons
They usually have weak bonds
Low melting points
Are poor conductors

Question 24

List the properties of metallic bonds and describe how they form

Answer 24

Form by bonding with the “sea” of electrons around other metals
They are lustrous
Ductile
Malleable
High melting points
Excellent conductors

Question 25

List the seven diatomic molecules and describe why they are diatomic

Answer 25

H2, N2, O2, F2, Cl2, Br2, I2 They are diatomic because they cannot exit alone in nature, so they must bond with another atom of the same element

Question 26

Linear model: 2 electron domain version (describe and list amount of shared pairs, unshared pairs, bond angles, electron domains, and hybridization)

Answer 26

2 shared pairs 0 lone pairs Straight line (180 degree bond angle) 2 electron domains Hybridization: sp

Question 27

Linear model: 1 electron domain version (describe and list amount of shared pairs, unshared pairs, bond angles, electron domains, and hybridization)

Answer 27

1 shared pairs 0 lone pairs Straight line (180 degree bond angle) 1 electron domains Hybridization: s Example: H2

Question 28

Trigonal Planar : (describe and list amount of shared pairs, unshared pairs, bond angles, electron domains, and hybridization)

Answer 28

3 shared pairs 0 lone pairs (120 degree bond angle) 3 electron domains Hybridization: sp2

Question 29

Bent model: 3 electron domain version (describe and list amount of shared pairs, unshared pairs, bond angles, electron domains, and hybridization)

Answer 29

2 shared pairs 1 lone pairs (<120 degree bond angle) 3 electron domains Hybridization: sp2 Electron geo: trigonal planar Molecular shape: bent

Question 30

Tetrahedral model (describe and list amount of shared pairs, unshared pairs, bond angles, electron domains, and hybridization)

Answer 30

4 shared pairs 0 lone pairs (109.5 degree bond angle) 4 electron domains Hybridization: sp3

Question 31

Trigonal Pyramidal (describe and list amount of shared pairs, unshared pairs, bond angles, electron domains, and hybridization)

Answer 31

3 shared pairs 1 lone pairs (<109.5 degree bond angle) 4 electron domains Hybridization: sp3 Molecular shape: trigonal pyramidal Electron geo: tetrahedral

Question 32

Bent: 4 electron domain version (describe and list amount of shared pairs, unshared pairs, bond angles, electron domains, and hybridization)

Answer 32

2 shared pairs 2 lone pairs (<109.5 degree bond angle) 4 electron domains Hybridization: sp3 Molecular shape:bent Electron geo: tetrahedral

Question 33

Name the following compounds Li3N

Answer 33

Lithium Nitride

Question 34

K3PO4

Answer 34

Potassium Phosphate

Question 35

NiCl3

Answer 35

Nickel (III) Chloride

Question 36

P4S5

Answer 36

Tetraphosphrous pentasulfide

Question 37

Si2Br6

Answer 37

Disilicon hexabromide

Question 38

Explain why storms seek out other atoms for chemical bonding

Answer 38

To achieve electron stability (full valence energy level), like the Noble gases

Question 39

Compare and contrast single, double, and triple bonds

Answer 39

Single bonds: co brain one shared pair of electrons, are weak, and are the greatest in length (all sigma bonds)

Question 40

Double bonds

Answer 40

Contain 2 shared pairs of electrons and have a strength and length between single and triple bonds (1 sigma bond, 1 Pi bond)

Question 41

Triple bonds

Answer 41

Continue 3 shared pairs of electrons, are very strong, and ate te shortest in length (1 sigma bond, 2 pi bonds)

Question 42

Which of te 7 diatomic molecules contains the strongest bonds? How do you know?

Answer 42

N2, because it contains triple bonds

Question 43

What is the electronegativity difference range for a nonpolar covalent

Answer 43

0 or very close to 0

Question 44

What is the electronegativity difference range for a slightly polar covalent

Answer 44

0-0.4

Question 45

What is the electronegativity difference range for a definitely polar covalent

Answer 45

0.5-2.1

Question 46

What is the electronegativity difference range for an ionic

Answer 46

Anything > 2.1

Question 47

True or false, A bond in which the elctronegatvity difference is less than 1.9 is considered to be mostly covalent in charchter

Answer 47

True

Question 48

A ____________ covalent bond is a covalent bond in which the doing electrons are shared equally between te two atoms

Answer 48

Nonpolar

Question 49

A _________ covalent bond is a covalent bond in which the atoms have an unequal attraction for electrons and so the sharing is unequals (don’t cancel)

Answer 49

Polar

Question 50

Describe the process for writing a chemical formula for an ionic bond

Answer 50

Find the oxidation number for each ion Criss cross the oxidation numbers Reduce if necessary

Question 51

What do you have to do with Polyatomic ions when surging their chemical formulas

Answer 51

Put them in paranethesis and do not chnage their subscripts or names

Question 52

What must your do to the end of an element snake when it is the second element in a compound

Answer 52

Chnage it to -ide

Question 53

Which lame ents require the Roman numerals in paranethese for making them? And what do they represent?

Answer 53

Transition mental, represents oxidation number

Question 54

What types of bonds require prefixes for naming the compound?

Answer 54

Covalent only