Name _________________________________________ Date __________________________ Period ____
Homework and Test Grade Recovery
Chapter 1: Introduction: Matter and Measurement
Exercises: Sections 1.2 and 1.3: Classification and Properties of Matter
1. Give the state of matter (gas, liquid, or solid) for each of the following under ordinary conditions of temperature and pressure:
(a) the element zinc; (b) the element neon; (c) octane, C8H18, which boils at 125oC (d) butane, which boils at ─ 0.5oC
(e) elemental iodine which sublimes at room temperature (f) water (g) mothballs (p-dichlorobenzene) which freezes at 52.85oC
Please write capital L, S, or G.
__________ (a)
__________ (f)
__________ (b)
__________ (c)
__________ (d)
__________ (e)
__________ (g)
2. Classify each of the following as a pure substance, P, or a mixture, M, and then indicate whether it is homogeneous, H, or
heterogeneous, HT:
(a) brass
(b) tomato juice
Pure Substance
or
Mixture
3.
(c) iodine crystals
Homogeneous
or
Heterogeneous
(d) soil
Pure Substance
or
Mixture
Homogeneous
or
Heterogeneous
__________
__________ (a)
__________
__________ (c)
__________
__________ (b)
__________
__________ (d)
(a) Is sand a heterogeneous or homogeneous substance?, how about sucrose (table sugar) C12H12O11?
(b) Is a mixture of sugar and sand homogeneous or heterogeneous?
(c) Explain how you determined the answer to part (b)
(d) Suggest a way to separate and recover each of the components in a mixture of sugar and sand.
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4. Without looking at a periodic table, write the chemical symbols for the following elements:
(a) carbon, (b) sodium, (c) fluorine, (d) iron, (e) phosphorus, (f) potassium, (g) nickel, (h) silver.
__________ (a)
__________ (b)
__________ (f)
__________ (g)
5.
__________ (c)
__________ (d)
__________ (e)
__________ (h)
Without looking at a periodic table, write the name each of the following elements:
(a) Co, (b) I, (c) Kr, (d) Hg, (e) As, (f) Ti, (g) K, (h) Ge.
__________ (a)
__________ (b)
__________ (c)
__________ (d)
__________
(e)
__________ (f)
__________ (g) __________ (h)
6. In 1807 the English chemist Humphry Davy passed an electric current through molten potassium hydroxide and isolated a bright,
shiny reactive substance. He claimed the discovery of a new element, which he named potassium. In those days, before the
advent of modern instruments, what was the bases on which one could claim that a substance was an element?
Scientists subjected the substance to all known chemical means of decomposition, and if the results were
negative the substance was classified as an element.
7. Explain the difference between chemical properties and physical properties. List some examples of
Each type of property
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8. Read the following description of the element zinc, and list the physical properties and chemical
properties.
Zinc (Zn) is a silver-gray colored metal, which melts at 420oC. When zinc granules are added to dilute
sulfuric acid(H2SO4) , hydrogen gas (H2) is given off and the metal dissolves. Zinc has a hardness on the
Mohs scale of 2.5 and a density of 7.13 g/cm3 at 25oC. It reacts slowly with oxygen gas (O2) at elevated
temperatures to form zinc oxide, ZnO.
Physical
Properties
Chemical
Properties
9. Explain the difference between chemical changes and physical changes. List some examples of each type of
change.
10. A match is lit and held under a cold piece of metal. The following observations are made:
(a) The match burns. (b) The metal gets warmer. (c) Water condenses on the metal.
(d) Soot (carbon) is deposited on the metal.
Which of these occurrences are due to physical changes (PC), and which are due to
chemical changes (CC)?
__________ (a)
__________ (b)
__________ (c)
__________ (d)
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11. A beaker contains a clear, colorless liquid. If it is water, how could you determine whether it contained
dissolved table salt? Do not taste it!
12. Define each of the following and then list some examples of each:
(a) Intensive properties
(b) Extensive properties
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Classification of Matter
MATTER
Pure Substances
(fixed composition)
Mixtures
(variable composition)
Elements
Simple
Suspensions
Colloids
Solutions
Heterogeneous
Large particle
Sand
Concrete
Granite
Compounds
Homogeneous
Small particles
muddy water
dusty air
blood
aerosol sprays
tomato juice
milk
jello
clouds
fog
smoke
mayonnaise
Submicroscopic particle
liquid in liquid = gasoline (mixture of hydrocarbon compounds)
solid in liquid = sea water (NaCl and other salts in water)
gas in liquid = soda pop (CO2 in water)
gas in gas = air (N2, O2, Ar, CO2, other gases)
as in solid = H2 in platinum or palladium
solid in solid = alloys (brass [Cu/ Zn], solder [Sn/ Pb])
liquid in sold = dental amalgams (mercury in silver)
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