Chemistry Test

Question 1

What is kinetic energy?

Answer 1

The energy due to motion

Question 2

What is kinetic theory?

Answer 2

all matter is made of particles in motion and the rate dictates the temperature.

Question 3

What is an intermolecular force?

Answer 3

An attraction between two separate molecules

Question 4

What is incorrect about “hydrogen bonds”?

Answer 4

Hydrogen bonds aren’t actually bonds, like (ionic and covalent), they are attractions. There is a polarity in the molecule

Question 5

Regarding gases, what is an “elastic collision”?

Answer 5

Elastic Collision: a collision where no kinetic energy is lost after a regular collision.

Question 6

What does STP refer to?

Answer 6

Standard Temp and Pressure

Question 7

What causes a gas to have pressure?

Answer 7

When particles hit the sides of a container (balloon)

Question 8

Why does pressure increase when temperature increases?

Answer 8

it increases because the particles have more energy when it is hotter, creating more collisions. (more pressure) (hitting sidewalls) (balloon)

Question 9

What are the three different types of motion?

Answer 9

Vibration,(moving in one spot) rotation,(spinning in place) and translation. (sliding side to side)

Question 10

What types of motion are observed in each of the three states of
matter (solid, liquid, gas)?

Answer 10

Solids=vibration, liquids=vibration and rotation, gases have all three.

Question 11

What is a fluid? Why do fluids flow?

Answer 11

A fluid: is a liquid or a gas, they flow, and have the ability to shape to the container they are in.

Question 12

How do intermolecular forces vary between the three states of
matter?

Answer 12

Solids have the strongest intermolecular forces, Liquids have some but gases have NONE.

Question 13

What is a change of physical state? What are three examples?

Answer 13

when energy is either added or subtracted changing the amount of intermolecular forces,

Question 14

What happens to intermolecular forces in a solid when it reaches
the melting point?

Answer 14

When heat is added, the energy destabilizes the force that holds them together. the energy breaks the particles holding it together.

Question 15

How is energy involved in a change of state?

Answer 15

When energy is added it pulls the particles apart and it decreases the intermolecular forces. And when it is removed the intermolecular forces move together.

Question 16

What is entropy? How is it involved in changes of state?

Answer 16

Entropy changes when temperature changes. When liquids turn into gas etc, this is an example of entropy.

Question 17

What is the heat of fusion? What does it mean for melting and freezing?

Answer 17

Energy that breaks away particles in a solid, or energy removed to allow liquids to become into solids.

Question 18

What is the heat of vaporization? What does it mean for boiling and condensing?

Answer 18

The same thing as Heat Of fusion however can turn liquids into gas, or gas into liquids.

Question 19

What is the representative unit for an ionic compound? What is it for a covalent compound?

Answer 19

Ionic: Formula unit
Covalent: Molecule unit

Question 20

30. What is a way to decide if a bond is ionic or covalent?

Answer 20

If it is IONIC: will have a metal
Covalent: will not have a metal

Question 21

31. What are three contrasts (or more) between ionic and covalent compounds?

Answer 21

Ionic: Have high melting points, high boiling points, are solids.
Covalent: Low melting points,low boiling points, are liquids or gases.

Question 22

What is meant by delocalized electrons?

Answer 22

electrons that are the outcome of metal and valence electrons, that are loose because there is no attraction, so there is more energy to move about

Question 23

Why do delocalized electrons matter for the properties of metals?

Answer 23

Loose electrons cause unique behaviors of the metals. (tin foil sheets solid, and can be rolled but also crunched)

Question 24

What is the definition for Luster?

Answer 24

how light interacts with a material

Question 25

What is the definition for Malleability?

Answer 25

When a material can be shaped into different things (foil)

Question 26

What is the defintion for Ductility?

Answer 26

When a material can be pulled into a small thin peice (like a wire)

Question 27

What is the definition for Conductivity?

Answer 27

When a material can transfer heat and electricity

Question 28

What is an alloy and why are they important?

Answer 28

A solution when different materials are blended and melted. AKA (the outcome of brass and steel) Important: more practical uses when in this formula than when seperate.

Question 29

What is a hydrogen bond? How does it contribute to surface tension?

Answer 29

When a polar/negative side of a molecule has attraction to electronegative atoms. Causes them to hold together better. (Why water from a spill is drawn into a paper towel)

Question 30

How does hydrogen bonding influence the melting/freezing and boiling/condensing points of water?

Answer 30

Water has extra strong intermolecular forces making it harder to break apart when it melts, freezes, boils, and condenses.

Question 31

Why is it odd that frozen water (ice) floats on the liquid water?

Answer 31

Most solids are dense than the liquid their formed from, but these solids are more dense because because the bonds spread the crystals out more than others do.

Question 32

What is an aqueous solution?

Answer 32

A solution where water is the solvent

Question 33

What are solutes and solvents?

Answer 33

Solute: A material that gets dissolved (koolaid-powder Solute: The one that does the dissolving (koolaid in WATER)

Question 34

What happens during the dissolving process?

Answer 34

solutes and solvents break apart from eachother and are blended into the solvent.

Question 35

How is an electrolyte different from a non-electrolyte?

Answer 35

Electrolyte: Conducts electricity Non-Electrolyte: Doesn't conduct electricity

Question 36

43. What are the three factors that affect the RATE at which a solution will be formed? What do they have in common?

Answer 36

Temperature- Heating will make a solvation happen faster Stirring-Solute will break down faster Particle Size- Small cubes have less mass so will dissolve faster (loose sugar vs sugar cube)

Question 37

What is solubility?

Answer 37

The amount of a solute that can be absorbed by a solvent with a specific temp and pressure

Question 38

Define unsaturated, saturated, and supersaturated solutions.

Answer 38

Unsaturated- not holding all the solute it could: Could be more dissolved Saturated- holding as much solute that it could (full) Supersaturated- A solvent is holding more of the normal amount it should be (overfull)

Question 39

What is the difference between a saturated solution and a concentrated solution?

Answer 39

Saturated: Holds all the solute possible Concentrated: Holds large amount but a little could be added ( the stage before Saturated)

Question 40

How does a solubility curve work?

Answer 40

The amount of solute that can dissolve in a solvent