1. Matter, Measurement, and The Language of Chemistry
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Unit 1
Matter, Measurement, and The Language of Chemistry

2. Matter Matter – anything that has mass and occupies space.
Matter can be classified according to its state (solid, liquid or gas.)

3. Matter (continued)
Matter can also be classified according to its composition:

4. Matter (continued)
Pure Substance – Composed of only a single type of atom or molecule.
Element – Composed of only one type of atom. Cannot be chemically broken down into simpler substances.
Compound – Composed of two or more elements in fixed, definite proportions.
Mixture – Composed of two or more different types of atoms or molecules that can be combined in variable proportions.

5. Heterogeneous Mixtures
A heterogeneous mixture consists of visibly different substances.

6. Homogeneous Mixtures
A homogeneous mixture has the same uniform appearance and composition.

7. Properties of Matter
Physical Properties – Characteristics of a substance that you can observe.
Examples: mass, volume, color, shape, odor, texture, melting point, boiling point, density.
Chemical Properties - Characteristics of a substance that describe how it can be changed into a new substance.
Examples: flammability, corrosiveness, reactivity, acidity, toxicity.

8. Changes in Matter
Physical Change – A change in physical properties, it is still the same substance.
Chemical Change – The change of a substance into a new, different substance.

9. Metric Measurement
Metric System – The standard measurement system used by scientists around the world. Also called the International System of Units, or SI. It is a decimal system, based on the number 10 and multiples of 10.

10. Length The basic metric unit of length is the meter (m).
A meter is a little longer than a yard.  A meter is a typical height for a 3-year old child, or about the size of two cocker spaniels.

11. Mass
The basic metric unit of mass is the gram (g). Mass is measured with a balance.
A gram is small. A nickel coin has a mass of about 5 g.
To measure larger amounts of mass, a kilogram (kg) is usually used. A kg is bigger than a pound. A 132 lb. person would have a mass of 60 kg.

12. Temperature oC = (oF -32) / 1.8 K = oC + 273
The SI unit for temperature is the kelvin (K).
Absolute zero – 0 K (-273oC) the coldest temperature possible, where all molecular motion stops.
You can convert between temperature scales with the following formulas:
oC = (oF -32) / 1.8
K = oC + 273

13. Volume The basic metric unit of volume is the liter (L).
One milliliter (ml) is the same as one cubic centimeter (cm3.)
2 L is the common size for a bottle of soda.
1 ml doesn’t even fill up a teaspoon.

14. Density
Extensive Properties depend on the amount of the substance. Examples: Mass, Volume.
Intensive Properties (also called characteristic properties) are independent of the amount of the substance. They can be used to identify substances. Example: Density.
Density is the ratio of mass to volume:
Density = Mass
Volume

15. Significant Figures
the non-place-holding digits in a reported measurement are called significant figures.
All non-zero numbers are significant, but some zeros in a written number are only there to help you locate the decimal point.
How do you remember which zeros are significant and which are not?

16. Significant Figures The Atlantic – Pacific Rule: Pacific (Present) -
If decimal point is present, start with the first non-zero number on the left.
Atlantic (Absent) -
If decimal point is absent, start with the first non-zero number on the right.

17. Significant Figures Examples: How many significant figures? 99,000
2 sig figs
99,000.
5 sig figs
0.0099
2 sig figs
0.0990
3 sig figs

18. Calculating with Significant Figures
When you use your measurements in calculations, your answer may only be as exact as your least exact measurement.
For addition and subtraction, round to the fewest decimal places.
Example: (3 decimals) (1 decimal) (unrounded) (rounded) =
67.7
For multiplication and division, round to the fewest significant figures.
Example: (3 sigfigs) (1 sigfig) (unrounded) (rounded)
x = 3

19. Uncertainty in Measurement
Uncertainty comes from limitations of measuring devices, experimental design, experimenter, and nature’s random behavior.
Accuracy – how close a measurement comes to the actual value.
Precision – how close measurements are to one another, or how reproducible they are.
Not Accurate and Not Precise
Accurate but Not Precise
Not Accurate but Precise
Accurate and Precise

20. Accuracy vs. Precision

21. Chemical Formulas octane — C8H18 aluminum sulfate — Al2(SO4)3
A chemical formula indicates the number of each kind of atom in a chemical compound.
when there is no subscript next to an atom, the subscript is understood to be 1.
Examples:
octane — C8H18
aluminum sulfate — Al2(SO4)3
there are 18 hydrogen atoms in the molecule.
there are 8 carbon atoms in the molecule.
Parentheses surround the polyatomic ion to identify it as a group. There are 3 SO4- groups.
there are 2 aluminum atoms in the formula unit.

22. Chemical Formulas Sample Problem
Count the number of atoms in the following chemical formulas:
Solution:
Ca(OH)2
KClO3
NH4OH
Fe2(CrO4)3
1 Calcium,
2 Oxygens,
and 2 Hydrogens
1 Potassium,
1 Chlorine,
and 3 Oxygens
1 Nitrogen,
5 Hydrogens,
and 1 Oxygen
2 Irons,
3 Chromiums,
and 12 Oxygens

23. Metals and Nonmetals
Metals tend to form positive (+) ions, Nonmetals tend to form negative (-) ions.

24. Monoatomic Ions Monoatomic Ions are ions formed from a single atom.
Some main-group elements tend to form covalent bonds instead of ions (ex. C and Si.) +1 +2 +3 -3 -2 -1

25. Monoatomic Ions Sample Problem
Identify each element as either a metal or a nonmetal. For main group elements, specify the ion that will form:
Metal or Nonmetal: Ion: Na Cu O Au Ba H N Al
metal +1
metal
nonmetal -2
metal
metal +2
nonmetal +1
nonmetal -3
metal +3

26. Chemical Categories by Formula
Ionic Compounds – Formed from metal (+) ions and nonmetal (-) ions.
Base – formula ends with the hydroxide ion (OH-1) (ex. KOH, Ca(OH)2, Al(OH)3)
Metallic Oxide – consists of only 2 elements: 1 metal and oxygen (ex. Na2O, MgO, SnO2)
Oxysalt – contains the element oxygen in the form of a polyatomic ion (ex. MgSO3, Ni(ClO3)2)
Salt – an ionic compound that can’t be classified into a more specific category (ex. NaCl, CuBr2)

27. Chemical Categories by Formula (continued)
Molecular Compounds – Formed from two or more nonmetals.
Non-metallic Oxide – consists of only 2 elements: 1 nonmetal and oxygen (ex. CO2, SO3, P4O10)
Hydrocarbon – consists of only 2 elements: carbon and hydrogen (ex. CH4, C2H4, C3H8)
Acids – formula begins with hydrogen (H+).
Binary acid – contains hydrogen and one other element (ex. HCl, H2S, HBr)
Oxyacid – contains oxygen in a polyatomic ion (ex. HNO3, H2SO4, H3PO4)

28. Chemical Categories by Formula Sample Problem
To which category does each of the following chemical formulas belong?:
Category:
BaSO3
Ag2O
Ca(OH)2
NiF2
C4H10
HNO2
PO5 HF
oxysalt
metallic oxide
base
salt
hydrocarbon
oxyacid
nonmetallic oxide
binary acid

29. Nomenclature Flowchart
Compounds
Compounds
Ionic
Ionic
Molecular
Acids
Prefix System
Hydro-carbons
Binary Acids
Oxyacids
Binary
Binary
Hydrates
Polyatomic Ions

30. Naming Binary Ionic Compounds
Binary Compounds are composed of 2 elements.
The name of the metal (+) ion is given first, followed by the name of the nonmetal (-) ion.
The first element in the compound is identified simply by its name.
For the second element, the ending of the its name is dropped, and the ending -ide is added.
Examples:
Al2O3
aluminum
oxide KF
potassium
fluoride

31. Writing Binary Ionic Compounds
Rules for writing binary ionic compounds:
Write the symbols for the ions, and their charges. Remember: The metal (+) ion is always written first.
Cross over the charges (use the absolute value of each ion’s charge as the subscript for the other ion.)
Simplify the numbers and remove the 1’s.
Example: aluminum oxide
The correct formula for aluminum oxide is
Al3+
O2– 2 3
Al2O3

32. Binary Ionic Compounds Sample Problem
Write chemical formulas for :
Magnesium Iodide
Calcium Oxide
Write the correct names for:
Li2S
ZnCl2
Solution:
Mg2+
I –
MgI2 1 2
Ca2+
O 2–
CaO 2 2
Hint: Always divide subscripts by their largest common factor .
Lithium Sulfide
Lithium
Zinc Chloride
Zinc

33. The Stock System
Most d-block elements (transition metals) can form 2 or more ions with different charges.
To name ions of these elements, scientists use the Stock system, designed by Alfred Stock in 1919.
The system uses Roman numerals to indicate an ion’s charge.
Example: Fe2+
Fe3+
iron(II)
iron(III)

34. Stock System Naming Sample Problem A
Write the formula and give the name for the compound formed by the ions Cr3+ and F–. Solution: Write the ions side by side, cation first. Cross over the charges to give subscripts. Chromium forms more than one ion, so its name must include the charge as a Roman numeral.
Cr3+
F – 1 3
CrF3
Chromium (III)
Fluoride

35. Stock System Naming Sample Problem B
Write chemical formulas for :
Tin (IV) Iodide
Iron (III) Oxide
Write the correct names for:
VF3
CuO
Solution:
Sn4+
I –
SnI4 1 4
Fe3+
O 2–
Fe2O3 2 3 3+ - V F3
Vanadium (III)
Fluoride 2 + - 2 Cu O
Copper (II)
Oxide
Hint: “Uncross” subscripts to get the charges of the ions.
Be sure to verify the charge of the anion.

36. Nomenclature Flowchart
Compounds
Compounds
Ionic
Ionic
Molecular
Acids
Prefix System
Hydro- carbons
Binary Acids
Oxyacids
Binary
Hydrates
Polyatomic Ions
Polyatomic Ions

37. There are 3 sulfate ions in this compound
Polyatomic Ions
Common Polyatomic Ions
A polyatomic ion is a charged group of covalently bonded atoms.
Common endings are -ate or -ite, but there are exceptions.
For more than 1 polyatomic ion, use parentheses with the subscript on the outside.
Example: Al2(SO4)3
There are 3 sulfate ions in this compound

38. Polyatomic Ions Sample Problem
Write chemical formulas for :
Calcium Hydroxide
Tin (IV) Sulfate
Write the correct names for:
(NH4)3 PO4
Cu(NO3)2
Solution:
Ca2+
OH –
Ca(OH)2 1 2
Sn4+
SO4 2–
Sn(SO4)2 2 4
Hint: Remember to divide subscripts by their largest common factor .
Ammonium
Phosphate - 2+ Cu
(NO3)2
Copper(II)
Nitrate
Hint: “Uncross” subscripts to get the charges of the ions.

39. Nomenclature Flowchart
Compounds
Compounds
Ionic
Ionic
Molecular
Acids
Prefix System
Hydro- carbons
Binary Acids
Oxyacids
Binary
Hydrates
Hydrates
Polyatomic Ions

40. Hydrates
Prefix
No. of Waters
hemi
mono 1 di 2
tri 3
tetra 4
penta 5
hexa 6
hepta 7
octa 8
Hydrates – ionic compounds that contain a specific number of water molecules associated with each formula unit.
in formula, attached waters follow.
in name, attached waters indicated by adding “prefixhydrate” after name of ionic compound.
Example:
CoCl2∙ 6H2O
cobalt(II) chloride hexahydrate

41. Hydrates Sample Problem
Write chemical formulas for :
calcium sulfate hemihydrate
barium chloride hexahydrate
Write the correct names for:
CuSO4 • 5H2O
LiF • 4H2O
Solution:
CaSO4 • ½ H2O
BaCl2 • 6H2O
copper (II) sulfate
pentahydrate
lithium fluoride
tetrahydrate

42. Nomenclature Flowchart
Compounds
Compounds
Ionic
Molecular
Molecular
Acids
Prefix System
Prefix System
Hydro- carbons
Binary Acids
Oxyacids
Binary
Hydrates
Polyatomic Ions

43. The Prefix System
Molecular compounds are composed of covalently-bonded molecules.
The old prefix system is still used for molecular compounds.
Name the prefix, then the element. Anions end in -ide.
The prefix mono- usually isn’t used for cations.
Examples: P4O CO
tetraphosphorus
decoxide
carbon
monoxide

44. The Prefix System Sample Problem
Write chemical formulas for :
dinitrogen trioxide
carbon tetrabromide
Write the correct names for:
As2S3
PCl5
Solution:
N2O3
CBr4
diarsenic
trisulfide
phosphorus
pentachloride

45. Nomenclature Flowchart
Compounds
Compounds
Ionic
Molecular
Molecular
Acids
Prefix System
Hydro- carbons
Hydro- carbons
Binary Acids
Oxyacids
Binary
Hydrates
Polyatomic Ions

46. Hydrocarbons
Hydrocarbons are compounds that contain only carbon and hydrogen.
Most fuels are mixtures of hydrocarbons.
Hydrocarbons containing only single bonds are called alkanes. Naming is based on the number of carbons , and the suffix –ane is added.
Base Name
No. of C
meth- 1
hex- 6
eth- 2
hept- 7
prop- 3
oct- 8
but- 4
non- 9
pent- 5
dec- 10

47. Hydrocarbons Sample Problem
Write chemical formulas for :
methane
butane
Write the correct names for:
C2H6
C3H8
Solution:
CH4
C4H10
ethane
propane

48. Nomenclature Flowchart
Compounds
Compounds
Ionic
Molecular
Acids
Acids
Prefix System
Hydro- carbons
Binary Acids
Binary Acids
Oxyacids
Oxyacids
Binary
Hydrates
Polyatomic Ions

49. Acids
An acid is a certain type of molecular compound. All acids start with H (e.g. HCl, H2SO4).
Acids can be divided into two categories:
Binary acids are acids that consist of H and a non-metal. (e.g. HCl.)
Oxyacids are acids that contain H and a polyatomic ion that includes O (e.g. H2SO4.)

50. Binary Acids General rules for naming a binary acid:
Begin with the prefix hydro-.
Name the anion, but change the ending to –ic.
Add acid to the name.
Examples:
HCl, hydrochloric acid.
HBr, hydrobromic acid.
H2S, hydrosulfuric acid.

51. Oxyacids General rules for naming an oxyacid :
Name the polyatomic ion.
Replace -ate with -ic or -ite with -ous
Add acid to the name.
Examples:
H2SO4, sulfuric acid.
H2SO3, sulfurous acid.
HNO3, nitric acid.
HNO2, nitrous acid.

52. Naming Acids Sample Problem
Write the correct name for each of the following: HF
HNO2
H2S
H2SO4
H3PO4
Type of Acid:
Name:
binary acid
hydro
fluorine
ic acid
oxyacid
nitrite
ous acid
binary acid
hydro
sulfur
ic acid
oxyacid
sulfate
uric acid
oxyacid
phosphate
oric acid

53. Heat and Temperature
Temperature – a measure of the average kinetic energy of the particles in a sample of matter.
The greater the kinetic energy of the particles in a sample, the hotter it feels.
Heat – energy transferred between samples of matter due to a difference in their temperatures.
Heat always moves spontaneously from matter at a higher temperature to matter at a lower temperature.

54. Measuring Heat
Heat energy is measured in joules (or calories – food only)
Chemical reactions usually either absorb or release energy as heat.
The energy absorbed or released as heat in a chemical or physical change is measured in a calorimeter.

55. Specific Heat
A quantity called specific heat can be used to compare heat absorption capacities for different materials.
Specific heat – the amount of energy required to raise the temperature of one gram of a substance by 1°C or 1 K.
Specific heat can be measured in units of J/(g•°C), J/(g•K), cal/(g•°C), or cal/(g•K).

56. Heat Transfer Equation
Specific heat can be used to find the quantity of heat energy gained or lost with a change in temperature according to the following equation:
Where the variables stand for the following: Q = heat transferred (joules or calories) m = mass (g) cp = specific heat ∆T = change in temperature (oC or K)
Q = m•cp•∆T

57. Heat Transfer Equation Sample Problem
A 4.0 g sample of glass was heated from 274 K to 314 K, a temperature increase of 40. K, and was found to have absorbed 32 J of energy as heat.
What is the specific heat of this type of glass?
b. How much energy will the same glass sample
gain when it is heated from 314 K to 344 K?
32 J
Q = m x cp x ∆T
cp = =
0.20 J/(g•K)
(4.0 g)
(40. K)
32 J =
(4.0 g)
(cp)
(40. K)
Q = m x cp x ∆T
Q =
(4.0 g)
(0.20 J/(g•K))
(30 K) =
24 J