Chapter 15 Test

Question 1

What are valence electrons?

Answer 1

The outermost electrons in an atom

Question 2

How do valence electrons relate to bonding?

Answer 2

These are in the outermost shells of atoms, so they are usually the only electrons involved with bonding.

Question 3

How do valences relate to group numbers? Is this true for all groups? Which groups is this true for?

Answer 3

They indicate the group number for groups 1A-8A, not the B groups

Question 4

What is a cation?

Answer 4

A positively charged ion formed when an atom loses electrons

Question 5

What kinds of elements are cations formed by and why do they do this?

Answer 5

Usually formed by metal atoms to achieve Noble Gas configurations and become stable

Question 6

What kinds of elements are stable? What makes them stable?

Answer 6

Noble gases are most stable, outer subshells are full

Question 7

What do all atoms want to do by common nature?

Answer 7

They want to adjust to achieve their lowest possible energy, their most stable energy state

Question 8

What is an anion?

Answer 8

A negatively charged ion formed when an atom gains electrons

Question 9

What kinds of elements are anions formed by and why do they do this?

Answer 9

Usually formed by nonmetal atoms to achieve Noble Gas configurations and become stable

Question 10

What is a monatomic ion?

Answer 10

A single atom ion with only one kind of element

Question 11

What is the suffix for monatomic ions?

Answer 11

-ide

Question 12

What are some examples of monatomic ions and their new names?

Answer 12

O-oxygen
O-2-oxide

F-fluorine
F-1-fluoride

Question 13

What is a polyatomic ion?

Answer 13

A group of different atoms with a charge. The group of atoms acts as a single unit.

Question 14

What are the endings for polyatomic ions?

Answer 14

-ite and -ate

Question 15

What is an example of a polyatomic ion?

Answer 15

CO2-carbon dioxide

CO3^-2-carbonate

Question 16

Who proposed the Octet Rule?

Answer 16

Lewis

Question 17

What is the Octet Rule?

Answer 17

Atoms react by changing the number of their electrons so as to acquire the stable electron structure of a noble gas

Question 18

What is the Octet Rule really an explanation of?

Answer 18

Why atoms tend to form their respective types of ions

Question 19

What is an ionic bond?

Answer 19

The force of attraction that bonds oppositely charged ions together

Question 20

What kind of forces are present in ionic bonds?

Answer 20

electrostatic attractions

Question 21

How does the ionic bonding relate to periodic trends?

Answer 21

Because nonmetals are smaller atoms with high EN and IE, they will pull off valence electrons from the metal atoms. they will gain electrons from metal atoms

Question 22

What do ionic bonds form?

Answer 22

Ionic compounds

Question 23

Why are all ionic compounds neutral?

Answer 23

The charges of anions plus the cation charges must equal 0.

Question 24

What is a formula unit?

Answer 24

The lowest whole number ratio of ions in an ionic compound which keeps the identity of that ionic compound

Question 25

What is a representative particle?

Answer 25

The smallest particle of a substance that keeps that substance's identity

Question 26

What are the representative particles for elements and compounds?

Answer 26

Atoms are the RPs for elements | Formula units are the RPs for the ionic compounds

Question 27

What are some properties of ionic compounds?

Answer 27

- composed of cations and anions | - electrically neutral charge, as cations and anions charges cancel each other

Question 28

When writing chemical formulas, which ion is writing first?

Answer 28

the cation

Question 29

What is the pattern structure of an ionic compound?

Answer 29

Crystal structure, repeating 3D pattern

Question 30

How do group B elements gain or lose electrons?

Answer 30

They lose outer electrons one at a time

Question 31

What is the coordination number? How does it relate to the atom's crystal structure?

Answer 31

The number of oppositely charged ions touching a single ion. The shape of the crystal is determined by the ion's charge and size.

Question 32

How does an ionic compound's crystal strength relate to how it conducts electricity?

Answer 32

It must have a free movement of charge to conduct electricity. Crystal structure means that ions are locked into a fixed position and unable to move freely, thus do not conduct electricity.

Question 33

What is the ionic compound's level of sturdiness?

Answer 33

They are brittle

Question 34

How are ionic compounds brittle?

Answer 34

When a force is applied to an ionic compound, like charges are forced together and in response, the like charges repel and the crystal shatters into smaller ones.

Question 35

What is the ionic compound's level of solubility?

Answer 35

Readily soluable in water

Question 36

How are ionic compounds readily soluable in water?

Answer 36

They are easily dissolvable in water; they dissocate (separate into individual ions)

Question 37

What is the ionic compound's property of melting point?

Answer 37

High melting point

Question 38

How do ionic compounds have a high melting point?

Answer 38

Determined by the strength of bonds, as bonds are strong, which raises the melting point, the stronger the bonds, the higher the melting point.

Question 39

What is the ionic compound's flammability property?

Answer 39

not flammable

Question 40

How are ionic compounds not flammable?

Answer 40

They will not combust when put in a flame.

Question 41

What is the ionic compound's conductor property?

Answer 41

They conduct in liquids

Question 42

How do ionic compounds conduct in liquids?

Answer 42

Liquid particles are more free to move around as more bonds break.

Question 43

Do ionic compounds conduct in solutions?

Answer 43

Yes

Question 44

Why do ionic compounds conduct in solutions?

Answer 44

Because ionic compounds dissocate when dissolved in water, the ions are free to move around and thus conduct electricity.

Question 45

What is a metallic bond?

Answer 45

The attraction between the free floating valence electrons and fixed positive nuclei of the metal atoms

Question 46

What are free floating valences called?

Answer 46

A sea of electrons

Question 47

Are metallic bonds malleable?

Answer 47

Yes

Question 48

How are metallic bonds malleable?

Answer 48

They are non-directional in their bonds

Question 49

How do metallic bonds work with many atoms?

Answer 49

The electrons in between can attract and slide over and attract to more than one atom

Question 50

Are metallic bonds ductile?

Answer 50

Yes

Question 51

What is an alloy?

Answer 51

A solution of metals

Question 52

Are metallic bonds good conductors?

Answer 52

Yes

Question 53

How are metallic bonds good conductors of heat and electricity?

Answer 53

The free floating valences cause them to slide over one another, attract to other nuclei and therefore transfer the heat and electricity from atom to atom

Question 54

What do metallic bonds conduct?

Answer 54

heat and electricity

Question 55

What are the two types of alloys?

Answer 55

substitutional alloys and interstitial alloys

Question 56

What are substitutional alloys?

Answer 56

Metal atoms in this alloy are the same size

Question 57

What are interstitial alloys?

Answer 57

Have metal atoms different in sizes at bonding, which causes for interstitial space, as the smaller atoms fit into these spaces

Question 58

Why are interstitial alloys more dense?

Answer 58

The smaller atoms fit into these interstitial spaces and cause for less room.

Question 59

How can you tell between hard and soft metals?

Answer 59

If an atom has 3 or more single "d" electrons, then they will bond and form a covalent network in addition to the metallic bonds, making them hard metals.

Question 60

What elements are the hard metals in the periodic table?

Answer 60

D3-D7 groups