Unit 4 Review

​Unit 4 Review

Matter​

Density is the amount of matter in a given volume.

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A dense material will sink in a less dense material.​

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​Unit 4: Matter Review

​Density Concept

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Multiple Choice

Density

• A metric unit of measurement used to measure small volumes of solid substances

• A physical property relating the amount of matter in a substance to the volume of the substance; a property used to identify and classify substances

• Has mass and takes up space; occurs as elements, compounds and mixtures

• Any form of matter that is uniform throughout and has consistent properties

Multiple Choice

Relative density

• D=m/v

• The comparison of the density of one material as it relates to another; frequently the comparison is to the density of water (as in sinking or floating)

• A procedure used to measure volume of a solid object by placing it in a known amount of liquid

• A metric unit of measurement used to measure small volumes of solid substances

Multiple Choice

Which box has a higher density?

• A

• B

• They are the same

• Unable to Determine

Density is the amount of matter in a given volume.

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A dense material will sink in a less dense material.​

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​Unit 4: Matter Review

​Density Calculations

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Multiple Choice

Find the density of a 2 cm x 2 cm x 2 cm cube with a mass of 64 g.

• 6 cm³
• 12 g/cm³
• 128 g/cm³
• 8  g/cm³

Multiple Choice

A diamond has a mass of 1.2 g.  If diamond has a density of 3.51 g/mL, what is the volume of the diamond.

• 0.34 mL
• 2.9 g/mL
• 2.3 mL
• 4.2 mL

Multiple Choice

Which TWO objects have the same DENSITY based from the table below?

• A and B

• A and C

• B and C

• B and D

A physical property can be observed with 5 senses and without changing the identity of the sample.

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A chemical property will change the material into a new substance.​

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​Unit 4: Matter Review

​Physical & Chemical Properties

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Multiple Choice

Physical properties....

• change the matter when studied

• can be observed and measured without changing the matter being studied

• include the ability to burn and rust

• are useless unless studied in a lab

Multiple Choice

If a substance has luster, it is ________

• shiny/reflective

• weak

• dull

• easily pulled into a wire

Multiple Choice

______________________ can only be recognized when substances react or do not react chemically with one another.

• Physical properties

• Chemical properties

• Flammable properties

• Colorful properties

Multiple Choice

Flammability means the ability to _______ and is a _________ property.

• melt; chemical

• rust; physical

• change; physical

• burn; chemical

Intermolecular Forces: force between molecules

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Intramolecular Forces: chemical bonds between atoms​

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​Unit 4: Matter Review

​Intermolecular Forces

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Multiple Choice

Forces that holds atoms together within the molecule

• intermolecular forces

• intramolecular forces

Multiple Choice

Forces that holds molecules together

• intramolecular forces

• intermolecular forces

Ion - Dipole

Water surrounding ions

Hydrogen Bonding

Hydrogen with F, O, N

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​Unit 4: Matter Review

​Intermolecular Forces Description

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Dipole - Dipole​

Polar Covalent Molecules​

London Dispersion Forces​

Non-polar Covalent Molecules​

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Multiple Choice

All molecules have London forces between them, but dipole-dipole and hydrogen bonding are so much stronger that when they are present we can ignore London forces.  Which of these has ONLY London forces?

• I₂
• NH₃
• OCl₂
• SH₂

Multiple Choice

________________________ have the strongest intermolecular forces of attraction.

• Dipole - Dipole

• London Dispersion

• Hydrogen Bonds

• Ion - Dipole

Multiple Choice

To form a hydrogen bonding, Hydrogen needs to attract to the highly electronegative elements such us _____, _____, and ____

• chlorine, fluorine, and oxygen

• fluorine, oxygen, and sulfur

• fluorine, bromine, and oxygen

• fluorine, oxygen, and nitrogen

Strong IMF

• Higher boiling point

• Higher viscosity

• Solid/Liquid​

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​Unit 4: Matter Review

​Intermolecular Forces & Properties

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Weak IMF

• Lower boiling point

• Lower viscosity

• Liquid/Gas​

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Multiple Choice

What explains the very high melting and boiling point of water

• Strong dipole-dipole bonds between water molecules
• Strong hydrogen bonds between water molecules
• Dispersion forces which are present in all molecules
• Asymmetrical shape of the polar bonds.

Multiple Choice

Which of the following statements correctly compares the behavior of a mixture of ethanol and water at STP?

• Water will evaporate first, because it has weaker intermolecular forces
• Ethanol will evaporate first, because it has weaker intermolecular forces
• Ethanol and water will evaporate simultaneously
• The aqueous solution will evaporate partially at a temperature between the boiling points of water and of ethanol

Multiple Choice

Which of the following statements correctly explains why hydrogen bonding is such a strong intermolecular force?

• There is an attraction between a small, weakly electronegative hydrogen atom and a large, strongly electronegative atom of fluorine, nitrogen, or oxygen
• There is an attraction between a small, highly electronegative hydrogen atom and a large, highly electronegative fluorine atom
• There is an attraction between the hydrogen and oxygen atoms, only
• There is an attraction between the hydrogen and nitrogen atoms, only

Multiple Choice

Which statement explains why Br₂ is a liquid at STP and I₂ is a solid at STP?

• Molecules of Br₂ are polar, and molecules of I₂ are nonpolar

• Molecules of Br₂ are nonpolar, and molecules of I₂ are polar

• Molecules of Br₂ have stronger intermolecular forces than molecules of I₂.

• Molecules of I₂ have stronger intermolecular forces than molecules of Br₂.