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Chemistry Test #1 > Chemistry Test > Flashcards

Chemistry Test Flashcards

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1
Q

What is kinetic energy?

A

The energy due to motion

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2
Q

What is kinetic theory?

A

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

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3
Q

What is an intermolecular force?

A

An attraction between two separate molecules

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4
Q

What is incorrect about “hydrogen bonds”?

A

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

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5
Q

Regarding gases, what is an “elastic collision”?

A

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

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6
Q

What does STP refer to?

A

Standard Temp and Pressure

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7
Q

What causes a gas to have pressure?

A

When particles hit the sides of a container (balloon)

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8
Q

Why does pressure increase when temperature increases?

A

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

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9
Q

What are the three different types of motion?

A

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

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10
Q

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

A

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

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11
Q

What is a fluid? Why do fluids flow?

A

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

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12
Q

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

A

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

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13
Q

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

A

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

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14
Q

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

A

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

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15
Q

How is energy involved in a change of state?

A

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.

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16
Q

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

A

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

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17
Q

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

A

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

18
Q

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

A

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

19
Q

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

A

Ionic: Formula unit
Covalent: Molecule unit

20
Q
  1. What is a way to decide if a bond is ionic or covalent?
A

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

21
Q
  1. What are three contrasts (or more) between ionic and covalent compounds?
A

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

22
Q

What is meant by delocalized electrons?

A

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

23
Q

Why do delocalized electrons matter for the properties of metals?

A

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

24
Q

What is the definition for Luster?

A

how light interacts with a material

25
Q

What is the definition for Malleability?

A

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

26
Q

What is the defintion for Ductility?

A

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

27
Q

What is the definition for Conductivity?

A

When a material can transfer heat and electricity

28
Q

What is an alloy and why are they important?

A

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.

29
Q

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

A

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)

30
Q

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

A

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

31
Q

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

A

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.

32
Q

What is an aqueous solution?

A

A solution where water is the solvent

33
Q

What are solutes and solvents?

A

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

34
Q

What happens during the dissolving process?

A

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

35
Q

How is an electrolyte different from a non-electrolyte?

A

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

36
Q
  1. What are the three factors that affect the RATE at which a solution will be formed? What do they have in
    common?
A

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)

37
Q

What is solubility?

A

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

38
Q

Define unsaturated, saturated, and supersaturated solutions.

A

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)

39
Q

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

A

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

40
Q

How does a solubility curve work?

A

The amount of solute that can dissolve in a solvent

Chemistry Test #1 (1 decks)

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