[CHEM] Unit 7- Bonding

Question 1

Breaking a bond is ___ (absorbs energy)

Answer 1

Endothermic

Question 2

Creating a bond is ___ (releases energy)

Answer 2

Exothermic

Question 3

Bonds create substances that have ___ potential ___ and ___ stability

Answer 3

Lower, energy, increased

Question 4

The octect rule:

Answer 4

Atoms are most stable with a full valence shell

Question 5

H, He, and Li have ___ valence electrons

Answer 5

2

Question 6

Be has ___ valence electrons

Answer 6

4

Question 7

B has ___ valence electrons

Answer 7

6

Question 8

T/F: The typical full shell of valence electrons IS NOT 8

Answer 8

F- the typical full shell is 8

Question 9

Nobles gases generally have a ___ valence shell and are ___

Answer 9

Full, unreactive

Question 10

T/F: Kr and ___ can bond with F

Answer 10

T- Kr and Xe can bond with F

Question 11

Metals have ___ valence electrons and low ___

Answer 11

Few, ionization energy

Question 12

The nucleus and ___ electrons (referred to as the “kernels”) form a crystal ___

Answer 12

Inner, lattice structure

Question 13

Ionic bonds, or electrovalent bonds, are a ___ bonded to a ___

Answer 13

Metal, nonmetal

Question 14

Ionic bonds generally have a electronegativity of ___ or more

Answer 14

1.7

Question 15

The solid of an ionic bond is a ___

Answer 15

Hard crystal lattice

Question 16

Ionic bonds have ___ melting and boiling points- generally in the ___

Answer 16

High, thousands

Question 17

Ionic bonds can only conduct electricity when ___ or ___

Answer 17

Liquid, aqueous

Question 18

Ionic bonds generally ___ in water

Answer 18

Dissolve

Question 19

The ___ difference in electronegativities, the ___ ionic the bond is

Answer 19

Greater, more

Question 20

The ___ pulls valence electrons ___ from the ___, making positive and negative ions which ___

Answer 20

Nonmetal, away, metal, attract

Question 21

Covalent bonds are:

Answer 21

Two nonmetals that bond; they share electrons

Question 22

Covalent bonds have an electronegativity that is ___ than 1.7

Answer 22

Less

Question 23

T/F: Covalent bonds CANNOT include atoms of the same element

Answer 23

F: they can

Question 24

T/F: Polyatomic ions are covalent

Answer 24

T

Question 25

T/F: Covalent bonds CANNOT exist in all three states of matter, and have HIGH boiling and melting points

Answer 25

F: They can exist in all three states, and have LOW melting and boiling points

Question 26

Covalent bonds are ___ and ___ conductors of electricity

Answer 26

Brittle, poor

Question 27

Nonpolar bonds are 2 atoms of the ___ element that share the valence electrons ___

Answer 27

SAME, EQUALLY

Question 28

Polar bonds are 2 atoms of ___ element(s) that share the valence electrons ___

Answer 28

DIFFERENT, UNEQUALLY

Question 29

MEMORIZE: Which elements have the highest electronegativities- in this specific order?

Answer 29

F,O,N,Cl

Question 30

Polar covalent bonds have electronegativities ___ than 1.7

Answer 30

Lower, smaller, less

Question 31

Ionic bonds have electronegativities ___ than 1.7

Answer 31

GREATER

Question 32

SNAP:

Answer 32

Symmetrical Nonpolar Asymmetrical Polar

Question 33

___ bonds are the easiest to break

Answer 33

Single

Question 34

___ bonds have the most bond energy

Answer 34

Triple

Question 35

A single bond is one ___ bond

Answer 35

Sigma

Question 36

A double bond is one ___ bond and one ___ bond

Answer 36

Sigma, pi

Question 37

A triple bond is one ___ bond and two ___ bonds

Answer 37

Sigma, pi

Question 38

A coordinate covalent bond is defined as:

Answer 38

Where both shared atoms come from the same source; ex: NH4+1 because N has five electrons and the two unpaired left over would go to the last H

Question 39

The general trend for hybridization is:

Answer 39

The hybridization is just sp_ whatever is one less than the number of bonding domains

Question 40

EVERYTHING IS ABOUT THE ___

Answer 40

CENTER ATOM

Question 41

Allotropes are:

Answer 41

2 forms of the same element but bonded differently, resulting in different physical and chemical purposes

Question 42

Network bonds/solids are:

Answer 42

A special case of covalent bonds which have very high melting points and are hard. The atoms are bonded by covalent bonds in a continuous network extending throughout the material. There are no individual molecules.

Question 43

Network bonds exist in a ___ ___ in which all of the atoms are bonded together ___

Answer 43

Crystal lattice, covalently

Question 44

Solubility rule:

Answer 44

“Like dissolves like”- for example, water and oil do not mix because water is polar and oil is nonpolar

Question 45

Polar solvents only dissolve ___ and ___ solvents because they ___ have charged parts

Answer 45

Ionic, polar, DO

Question 46

Nonpolar solvents only dissolve ___ solvents because they ___ have charged parts

Answer 46

Nonpolar, DO NOT

Question 47

T/F: Hydrogen bonding is the weakest of all IMFs (intermolecular forces) and has a low boiling point and low surface tension

Answer 47

F: This is false. Hydrogen bonds are the strongest of IMFs and have high boiling points and surface tension

Question 48

Hydrogen bonding only works when __, ___, or ___ bond with ___

Answer 48

F,O,N, H

Question 49

Dipole-dipole forces are between 2 ___ molecules and are ___ than hydrogen bonding

Answer 49

POLAR, weaker

Question 50

T/F: Van der Waals forces are the strongest of the IMFs

Answer 50

F: VdW forces are the WEAKEST

Question 51

Van der Waals forces are between ONLY ___ molecules or ___ ___

Answer 51

Nonpolar, noble gases

Question 52

VdW forces are created because:

Answer 52

Electrons move, creating temporary charges that attract molecules for short periods of time

Question 53

___ molecules lead to stronger VdW forces

Answer 53

Larger (heavier mass)