States & Phases of Matter
Physical & Chemical Properties/Changes
Density
Classifying Matter
Classifying Matter, Part II
100
Matter is anything that has _________ and __________.
mass; volume (or takes up space)
100
Which change produces a new substance, physical change or chemical change?
Chemical change
100
Density is the relationship between an object's ___ and ___.
Mass and density
100
What are the two main types of matter?
Pure substances and mixtures?
100
Which mixtures exhibit the Tyndall Effect? Be more specific than homogeneous and heterogeneous mixures.
Colloids and suspensions.
200
Describe the shape and volume of the three states of matter
Solid: definite shape and definite volume
Liquid: indefinite shape and definite volume
Gas: indefinite shape and indefinite volume
200
Define physical properties and list 5 physical properties.
Physical properties can be observed or measured without changing the substance. Solubility, density, polarity, malleability, ductility, etc.
200
Find the density of an object that has a mass of 525 g and occupies a volume of 15.0 mL.
35.0 g/mL
200
What are the two types of pure substances? Define and give an example of each.
Element - pure substance made up of only one kind of atom (ex: Hydrogen, Oxygen, etc.)
Compounds - pure substance made up of two or more elements chemically combined in set ratios (ex: NaCl, H2O, CO2)
200
True or False: When substance form mixtures, the substances do not retain their original properties.
False, they do.
300
Describe the kinetic energy of all three states of matter.
Solid - low KE, liquid - medium KE, gas - high KE
300
Define chemical properties and list the 4 that we've gone over.
Chemical properties describe matter based on its ability to change into new matter that has different properties. Ex: Toxicity, Reactivity, Oxidation state, and Flammability.
300
One side of a cube measures 4 cm long. The cube’s mass is 250 g. Find the density of the cube.
4 g/cm3
300
What are the two types of mixtures? Define and give an example of each.
Homogeneous mixtures - Mixture of two or more substances physically combined that appears uniform throughout (ex: solutions and colloids; salt water and milk)
Heterogeneous mixture - mixture of two or more substances physically combined that does NOT appear uniform. You can see the different parts. (ex: suspensions; salad dressing, cereal, etc.)
300
List 3 ways to increase the solubility of a solid
Stir it, shake it, heat it, crush it.
400
What is happening at parts 2 and 4?
Part 2 is a solid and a liquid, part 4 is a liquid and a gas. The substance is undergoing a phase change and the heat being added is used to help overcome that phase change.
400
Give 4 examples of physical changes.
Tearing a paper, crushing a can, changing state (ice melting, water freezing), dissolving salt in water, etc.
400
The density of copper is 8.96 g/mL. The sample of copper you have has a volume of 2.40 mL. Find the mass of the sample.
21.5 g
400
How can we classify mixtures even further? Define all 3 and give 1 example of each.
Solution - small particles, evenly distributed, does not scatter light. Ex: salt water, sugar in water
Colloids - medium particles, evenly distributed, DOES scatter light, can be opaque. Ex: milk, fog
Suspensions - large particles, particles settle, DOES scatter light, can be opaque, must shake! Ex: salad dressing, pulpy orange juice
400
What approximate mass of NaNO3 will dissolve in 100 g of water at 10 oC?
80 g
500
What is the melting point and the boiling point of this substance?
Melting: 0 oC
Boiling: 100 oC
500
Give 4 signs of a chemical change
Change in color, Change in odor, Production of gas (fizzing/foaming), Heat given off (exothermic), Heat taken in (endothermic), Light created, Sound produced, Precipitate forms
500
Water’s density is 1 g/mL. What would happen to a solid object with a density that is less than water when it is placed in water?
It would float.
500
Classify solutions even further and define each, using the words "solute" and "solvent" in your answer
Unsaturated: a solution that contains less solute than can be dissolved in the solvent. The solvent is capable of dissolving more solute if added.
Saturated: a solution containing as much solute as the solvent is capable of dissolving. Any additional solute added will collect at the bottom.
Supersaturated: a solution containing a greater solute than the solvent can hold. This occurs when a saturated solution is carefully cooled.
500
If you want to dissolve 40 g of KCl at 50 oC, will the solution be unsaturated or saturated?
Unsaturated