Honchem Unit 3 Exam

Front 1

How many main types of bonds are there?

Back 1

3

Front 2

Ionic Bond

Back 2

Between a metal and a nonmetal. In Ionic bonds, electrons are TRANSFERRED

Front 3

Metallic Bond

Back 3

Between a metal and a metal

Front 4

Covalent Bond

Back 4

Between nonmetals, electrons are SHARED

Front 5

Valence Electrons

Back 5

electrons on the outer shell of an atom

Front 6

Octet Rule

Back 6

All atoms "want" to obtain the electron configuration of a noble gas (8 valence electrons) except for Helium (2 valence electrons)

Front 7

Lewis Dot Diagram

Back 7

Dots to indicate the # of valence electrons in the outer shell

Front 8

What is the type of force that holds ions together in an ionic compound?

Back 8

electrostatic (opposites attract)

Front 9

Why are ionic compounds such poor conductors in solid form? Why can they conduct when dissolved in water?

Back 9

Ionic compounds are poor conductors in solid form because their bonds are very strong (strong attraction between + and - ions), so the electrons are unable to move and conduct. They can conduct in liquid form because the ions and electrons are free to move.

Front 10

Four properties of ionic compounds are...

Back 10

1. All solid at room temperature because they have strong bonds
2. Brittle
3. Bad conductors in solid form
4. Good conductors in liquid form

Front 11

Salt

Back 11

ANY ionic compound

Front 12

Halide

Back 12

a salt that contains a halogen

Front 13

Crystal Lattice

Back 13

A repetitive arrangement of atoms in an ionic compound

Front 14

Lewis Dot Diagram with Ionic Bonds

Back 14

Review this

Front 15

Metallic bonds must contain two different metals (T or F)

Back 15

F, because they can contain atoms of the same metal OR atoms of two different metals

Front 16

Properties of metals

Back 16

Conducts electricity, conducts heat, malleable, ductile, luster, all silver except for gold and copper

Front 17

In a metallic bond, the valence electrons form a...

Back 17

roving sea of electrons

Front 18

What is the roving sea of electrons?

Back 18

It allows the movement of the valence electrons

Front 19

In a metallic bond, the valence electrons "belong" to...

Back 19

ALL of the metal atoms

Front 20

What causes the metallic bond?

Back 20

Electrons are free to roam, this creates a positively charged side and a negatively charged, which are attracted to one another, hence forming a bond

Front 21

Alloy

Back 21

solid metal solution made up of two or more elements

Front 22

Covalent bond (more specific definition)

Back 22

2 or more valence electrons are shared between two atoms

Front 23

Single bond

Back 23

1 pair of electrons are shared between two atoms

Front 24

What creates a covalent bond?

Back 24

Positively charged nucleus attracted to electrons of another atom

Front 25

Electronegativity

Back 25

attraction of one atom for the electrons of another in a bond (highest Electronegativity: F)

Front 26

Nonpolar covalent bond

Back 26

when electrons are equally shared between two atoms (they are in the middle)

Front 27

Polar covalent bond

Back 27

When electrons are unequally shared (One atom is closer to the electrons)

Front 28

Dipole

Back 28

When a bond or molecule has unequal sharing

Front 29

The type of bond is determined by...

Back 29

the difference in electronegativities (Ionic bonds, difference is greater than or equal to 2.1, Polar Covalent bonds have a difference greater than or equal to 0.5, but less than 2.1, and Nonpolar covalent bond have a difference of 0 to 0.5

Front 30

How does a covalent bond differ from an ionic bond?

Back 30

Convalent bonds have a sharing of electrons while ionic bonds have a transfer of electrons

Front 31

Bond dissociation energy

Back 31

the energy required to break the chemical bond between two atoms and separate them

Front 32

Molecular shapes are based on...

Back 32

VSEPR (Valence, Shell, Electron, Pair, and Repulsion (electrons want to be as far apart as possible)

Front 33

In Lewis Structures, Hydrogen is always in the middle (T or F)

Back 33

F, because hydrogen wants only 2 electrons

Front 34

In Lewis Structures, Carbon is almost always in the middle (T or F)

Back 34

T

Front 35

Molecular Polarity depends on...

Back 35

Electronegativity difference and the molecular shape

Front 36

Bond Polarity depends on...

Back 36

Electronegativity difference

Front 37

Polarity only applies to...

Back 37

Covalent bonds, any non-metal to non-metal

Front 38

Intermolecular Forces

Back 38

Forces between molecules, attraction that exists between molecules, weaker than a bond

Front 39

Intramolecular Forces

Back 39

Forces within molecules (Covalent bonds)

Front 40

Hydrogen Bond

Back 40

A form of dipole attraction in which a hydrogen atom bonded to a strongly electronegative atom is attracted to another electron rich atom

Front 41

London Dispersion Force

Back 41

An attraction between atoms and molecules caused by the formation of instantaneous dipoles in the atoms and molecules (Non-polar molecules attracted to other non-polar molecules)

Front 42

Dipole Force (relating to intermolecular forces)

Back 42

between two polar molecules

Front 43

Hydrogen bonding

Back 43

Strong type of dipole bond, always between Hydrogen and FON (Fluorine, Nitrogen, or Oxygen)

Front 44

LDF's can have a strong total force when...

Back 44

There are large amounts of LDF's

Front 45

The larger the nonpolar molecule, the higher the ___________ because more electrons = more _______ = stronger force

Back 45

boiling point, LDF's

Front 46

Network Solids

Back 46

No intermolecular forces, all covalent bonds, only compounds of pure Carbon and Silicon + Oxygen and others

Front 47

Examples of Network Solids...

Back 47

Graphite, Diamonds, Quartz (SiO2)

Front 48

Ionic Bonds have a strength of...

Back 48

85

Front 49

Metallic bonds have a strength of...

Back 49

65

Front 50

Network solids have a strength of

Back 50

100 (the highest)

Front 51

Hydrogen Bonds have a strength of

Back 51

5

Front 52

Dipoles have a strength of

Back 52

1

Front 53

LDF's have a strength of

Back 53

0.1

Front 54

Which substance has a stronger bond? NaCl or H2O?

Back 54

NaCl, because it is an ionic bond with a strength of 85

Front 55

Fe or CH4

Back 55

Fe, because it is a metallic bond

Front 56

The stronger the bond, the higher the ____________ and the ___________

Back 56

melting point and boiling point

Front 57

Noble gasses are what type of forces?

Back 57

LDF's

Front 58

Why are valence electrons important?

Back 58

They determine the chemical properties of an element and they are the electrons involved in bonding