Inorganic & Organic Chemistry Reviewer
Lesson 1: Matter and Measurement
Differences between Inorganic and
Organic substances.
What is Chemistry?
Chemistry is too universal and Organic Inorganic
dynamically-changing a subject to be confined to a
Based on carbon Not based on carbon
fixed definition; it might be better to think of chemistry
more as a point of view that places its major focus on Nonelectrolyte Electrolyte
the structure and properties of substances—
particular kinds of matter— and especially on the Covalent bonding Ionic Bonding
changes that they undergo. Chemistry is the study of
Low boiling and High boiling and
matter— its composition, properties, and melting points melting points
transformations.
Soluble in nonpolar Soluble in polar
Chemistry: The Central Science solvents solvents
The real importance of Chemistry is that it
Complex structure Simple structure
serves as the interface to practically all of the other
sciences, as well as to many other areas of human
endeavor. For this reason, Chemistry is often said (at The Scientific Method
least by chemists!) to be the "central science". All science employ variations of what is called
Chemistry being the central science plays an the scientific method, a systemic approach to
important part in all other natural sciences, basic and research. Scientific method involves several steps:
applied. Plant growth and metabolism, the formation
of igneous rocks, the role played by ozone in the 1. Observation. As researchers are generally
atmosphere, the degradation of environmental curious about their surroundings, this curiosity leads
pollutants, the properties of lunar soil, the medical them to ask questions about the world around them.
action of drugs, establishment of forensic evidence:
None of these could be understood without the 2. Formulation of hypothesis (tentative
knowledge and perspective provided by chemistry. explanation for a set of observations).
Indeed, many people study chemistry so that they
can apply it to their own particular field of interest. 3. Testing of hypothesis, of all the steps in
scientific method, the one that truly separates
Chemistry: Inorganic and Organic science from other disciplines is the process of
Organic chemistry is the study of molecules experimentation. In order to prove, or disapprove, a
that contain carbon compounds. It studies the hypothesis, a scientist will design an experiment to
structure, properties, composition, and reactions test the theory.
of compounds that contain carbon. These •
molecules are related to substances produced by 4. Generalization. Concluding statements
living organism but it also includes human-made derived after hypothesis survive many experimental
substances such as plastics. Inorganic chemistry is tests of their validity which can be further tested and
the study of all compounds that do not contain carbon may evolve into theories.
compounds. Inorganic chemistry studies the
synthesis and behavior of the inorganic compounds What is matter?
which do not have C-H bond. Inorganic compounds Matter is anything that has mass and takes up
include salt, metals and substances made from volume.
only one inorganic such as fertilizers. It has
application in: Material science, Pigments, • Matter is anything that has volume and mass
Surfactants, Coatings, Medications, Fuels and • Volume is the amount of space taken up, or
Agriculture. occupied, by an object
,Inorganic & Organic Chemistry Reviewer
• Mass is the amount of matter that something Classification of matter
is made of.
1. PURE SUBSTANCE is composed of a single
2 TYPES OF MATTER component and has a constant composition,
Naturally occurring: like cotton, sand, and regardless of the sample size and origin of the
digoxin, a cardiac drug. sample. A pure substance cannot be broken down to
Synthetic (human-made): like nylon, another pure substance by any physical change.
Styrofoam and ibuprofen.
A pure substance is classified as either an
States of Matter element or a compound
1. Solid - has a definite volume, and - An ELEMENT is a pure substance that
maintains its shape regardless of the container in cannot be broken down into simpler substances by a
which it is placed. The particles of a solid lie close chemical reaction.
together and are arranged in a regular - A COMPOUND is a pure substance formed
three-dimensional array. by chemically combining (joining together) two or
2. Liquid - has a definite volume, but takes on more elements.
the shape of the container it occupies. The particles
of a liquid are close together, but they can randomly 2. MIXTURE is composed of more than one
move around, sliding past one another. component. The composition of a mixture can vary
3. Gas - has no definite shape or volume. The depending on the sample. A mixture can be
particles of a gas move randomly and are separated separated into its components by physical changes.
by distance much larger than their size. The particles
of a gas expand to fill the volume and assume the
shape of whatever container they put in.
Matter can be characterized by its PHYSICAL
and CHEMICAL properties. Physical properties are
those that can be observed or measured without
changing the composition of the material. Common
physical properties include melting point, boiling
point, solubility, color, and odor. A physical
change alters the substance without changing its
composition. The most common physical changes
are changes in state. Chemical properties are those Measurements are routine for healthcare
that determine how a substance can be converted to professionals who use weight, blood pressure, pulse,
another substance. A chemical change, or chemical and temperature to chart a patient’s progress. Every
reaction, converts one material to another. measurement is composed of a number and a unit.
The number is meaningless without the unit.
A PHYSICAL CHANGE is a change in appearance
only. The matter is still the same after the change The Metric System
takes place. Each type of measurement has a base unit - the
Examples: cutting paper, melting butter, meter (m) for length; the gram (g) for mass; the liter
dissolving salt in water, and breaking glass (L) for volume; the second (s) for time. All other units
A CHEMICAL CHANGE occurs when matter are related to the base unit by power of 10. The prefix
is changed into one or more different types of matter. of the unit name indicates if the unit is larger or
Examples: rusting, hydrogen and oxygen to smaller than the base unit.
water, fire, and overcooking
,Inorganic & Organic Chemistry Reviewer
The Basic Metric Units
Measuring Mass
Quantity Metric Base Unit Symbol • Mass is a measure of the amount of matter in
an object.
Length Meter m
• Weight is the force that matter feels due to
Mass Gram g gravity.
• The base unit of mass in the metric system is
Volume Liter L
the gram (g).
Time Second s 1 kilogram (kg) = 1,000 grams (g)
1 kg = 1,000 g
1 milligram (mg) = 0.001 grams (g)
Common Prefixes Used for Metric Units 1 mg = 0.001 g
Prefix Symb Meaning Numerical Scientific
ol Value Notation Measuring Volume
The base unit of volume in the metric system is the
Mega- M Million 1,000,000. 10⁵ liter (L).
Kilo- k Thousand 1,000. 10³
1 kiloliter (kL) = 1,000 liters (L)
Deci- d Tenth 0.1 10⁻¹ 1 kL = 1,000 L
Centi- c Hundredth 0.01 10⁻²
1 milliliter (mL) = 0.001 liters (L)
Mili- m Thousandth 0.001 10⁻³ 1 mL = 0.001 L
Micro- µ Million 0.000 001 10⁻⁶
VOLUME = Length x Width x Height
Nano- n Billionth 0.000 000 001 10⁻⁹ = cm x cm x cm
= cm3
Measuring Length
1 mL = 1 cm3 = 1 cc
The base unit for length is meter (m).
1 meter (m)
English Units and their metric equivalents
1 meter = 0.001 km
1 meter = 100 cm Quantity English Unit Metric-English
Relationship
1 meter = 1000 mm
Length 1 ft = 12 in. 2.54 cm = 1 In.
1 yd =3 ft 1 m = 39.4 In.
1 kilometer (km) 1 mi.= 5,280 ft 1 km = 0.621 mi
1 km = 1,000 m
1 km = 1,000,000 mm Mass 1 lb =16 oz 1 kg = 2.20 lb
1 ton = 2,000 lb 454 g = 1 lb
1 km = 100,000 cm 28.3 g = 1 oz
1 millimeter (mm) Volume 1 qt = 4 cups 946 mL = 1 qt
1 qt = 2 pints 1 L= 1.06qt
1 mm = 0.001 m 1 qt = 32 fl oz 29.6 mL =1 fl oz
1 mm = 0.1 cm 1 gal = 4 qt
Common abbreviations for English units: inch (in.). foot
1 centimeter (cm) (ft). yard (ycl). mile (m1). pound (lb). ounce (oz). gallon
1 cm = 0.01 m (gal). quart (qt) and fluid ounce (I1 oz).
1 cm = 10 mm
Example: how many liters is 1.0 pint of blood?
1 pint x 1qt/2pint x 1L/1.06qt
1 x ½ x 1L/1.06
, Inorganic & Organic Chemistry Reviewer
= 0.472 • Ex: 509 has 3 significant figures.
Significant Figures 3. A final zero or trailing zeros in the decimal portion
✓ An exact number results from counting objects is ONLY are significant.
part of a definition • Ex: .500 or .632000 the zeros are significant
✓ An inexact number results from a measurement or • .006 or .000968 the zeros are NOT significant!
observation and contains some uncertainly
✓ Significant figures are all the digits measured SIGNIFICANT FIGURES IN NUMERICAL
number including one estimate digit COMPUTATIONS
i. Sums and differences - for addition and
Determining the number of Significant subtraction, the result should have the same number
figures of decimal places as the number with the smallest
✓ All nonzero digits are always significant. number of decimal places.
Rules to determine when a zero is a ii. Products and quotients - assume unit uncertainty
significant figure: in the last digit of each number. - the least number of
Rule [1] A zero counts as significant Exa zeroample significant figures in any number of the problem
figure when it occurs: determines the number of significant figures in the
29.05g — four SF
answer.
• Between two non-zero digits
1.0087mL — five SF
• At the end of a number with
25.70 cm — four SF Example: 2.5 x 3.42
a decimal point
3.7500 — five SF - The answer to the problem would be 8.6
620. lb — three SF
- Why? 2.5 has two significant figures while 3.42 has
Rule [2] A zero does not count as a three.
significant figure when it
- Two significant figures is less precise than three, so
occurs:
the answer has two significant figures.
• At the beginning of a number 0.0245 mg — three SF
0.008 mL — one SF
• At the end of a number that
2,570 m — three SF
does not have a decimal point
1,245,500 m — five
SF
RULES FOR DETERMINING THE NUMBER OF
SIGNIFICANT FIGURES
i. Disregard all initial zeros.
ii. Disregard all final zeros unless they follow a
decimal point.
iii. All remaining digits including zeros between
nonzero digits are significant.
THERE ARE THREE RULES ON DETERMINING
HOW MANY SIGNIFICANT FIGURES ARE IN A
NUMBER:
1. Non-zero digits are always significant.
• Ex: 26.38 would have 4 significant figures and 7.94
would have 3.
2. Any zeros between two significant digits are
significant.
Lesson 1: Matter and Measurement
Differences between Inorganic and
Organic substances.
What is Chemistry?
Chemistry is too universal and Organic Inorganic
dynamically-changing a subject to be confined to a
Based on carbon Not based on carbon
fixed definition; it might be better to think of chemistry
more as a point of view that places its major focus on Nonelectrolyte Electrolyte
the structure and properties of substances—
particular kinds of matter— and especially on the Covalent bonding Ionic Bonding
changes that they undergo. Chemistry is the study of
Low boiling and High boiling and
matter— its composition, properties, and melting points melting points
transformations.
Soluble in nonpolar Soluble in polar
Chemistry: The Central Science solvents solvents
The real importance of Chemistry is that it
Complex structure Simple structure
serves as the interface to practically all of the other
sciences, as well as to many other areas of human
endeavor. For this reason, Chemistry is often said (at The Scientific Method
least by chemists!) to be the "central science". All science employ variations of what is called
Chemistry being the central science plays an the scientific method, a systemic approach to
important part in all other natural sciences, basic and research. Scientific method involves several steps:
applied. Plant growth and metabolism, the formation
of igneous rocks, the role played by ozone in the 1. Observation. As researchers are generally
atmosphere, the degradation of environmental curious about their surroundings, this curiosity leads
pollutants, the properties of lunar soil, the medical them to ask questions about the world around them.
action of drugs, establishment of forensic evidence:
None of these could be understood without the 2. Formulation of hypothesis (tentative
knowledge and perspective provided by chemistry. explanation for a set of observations).
Indeed, many people study chemistry so that they
can apply it to their own particular field of interest. 3. Testing of hypothesis, of all the steps in
scientific method, the one that truly separates
Chemistry: Inorganic and Organic science from other disciplines is the process of
Organic chemistry is the study of molecules experimentation. In order to prove, or disapprove, a
that contain carbon compounds. It studies the hypothesis, a scientist will design an experiment to
structure, properties, composition, and reactions test the theory.
of compounds that contain carbon. These •
molecules are related to substances produced by 4. Generalization. Concluding statements
living organism but it also includes human-made derived after hypothesis survive many experimental
substances such as plastics. Inorganic chemistry is tests of their validity which can be further tested and
the study of all compounds that do not contain carbon may evolve into theories.
compounds. Inorganic chemistry studies the
synthesis and behavior of the inorganic compounds What is matter?
which do not have C-H bond. Inorganic compounds Matter is anything that has mass and takes up
include salt, metals and substances made from volume.
only one inorganic such as fertilizers. It has
application in: Material science, Pigments, • Matter is anything that has volume and mass
Surfactants, Coatings, Medications, Fuels and • Volume is the amount of space taken up, or
Agriculture. occupied, by an object
,Inorganic & Organic Chemistry Reviewer
• Mass is the amount of matter that something Classification of matter
is made of.
1. PURE SUBSTANCE is composed of a single
2 TYPES OF MATTER component and has a constant composition,
Naturally occurring: like cotton, sand, and regardless of the sample size and origin of the
digoxin, a cardiac drug. sample. A pure substance cannot be broken down to
Synthetic (human-made): like nylon, another pure substance by any physical change.
Styrofoam and ibuprofen.
A pure substance is classified as either an
States of Matter element or a compound
1. Solid - has a definite volume, and - An ELEMENT is a pure substance that
maintains its shape regardless of the container in cannot be broken down into simpler substances by a
which it is placed. The particles of a solid lie close chemical reaction.
together and are arranged in a regular - A COMPOUND is a pure substance formed
three-dimensional array. by chemically combining (joining together) two or
2. Liquid - has a definite volume, but takes on more elements.
the shape of the container it occupies. The particles
of a liquid are close together, but they can randomly 2. MIXTURE is composed of more than one
move around, sliding past one another. component. The composition of a mixture can vary
3. Gas - has no definite shape or volume. The depending on the sample. A mixture can be
particles of a gas move randomly and are separated separated into its components by physical changes.
by distance much larger than their size. The particles
of a gas expand to fill the volume and assume the
shape of whatever container they put in.
Matter can be characterized by its PHYSICAL
and CHEMICAL properties. Physical properties are
those that can be observed or measured without
changing the composition of the material. Common
physical properties include melting point, boiling
point, solubility, color, and odor. A physical
change alters the substance without changing its
composition. The most common physical changes
are changes in state. Chemical properties are those Measurements are routine for healthcare
that determine how a substance can be converted to professionals who use weight, blood pressure, pulse,
another substance. A chemical change, or chemical and temperature to chart a patient’s progress. Every
reaction, converts one material to another. measurement is composed of a number and a unit.
The number is meaningless without the unit.
A PHYSICAL CHANGE is a change in appearance
only. The matter is still the same after the change The Metric System
takes place. Each type of measurement has a base unit - the
Examples: cutting paper, melting butter, meter (m) for length; the gram (g) for mass; the liter
dissolving salt in water, and breaking glass (L) for volume; the second (s) for time. All other units
A CHEMICAL CHANGE occurs when matter are related to the base unit by power of 10. The prefix
is changed into one or more different types of matter. of the unit name indicates if the unit is larger or
Examples: rusting, hydrogen and oxygen to smaller than the base unit.
water, fire, and overcooking
,Inorganic & Organic Chemistry Reviewer
The Basic Metric Units
Measuring Mass
Quantity Metric Base Unit Symbol • Mass is a measure of the amount of matter in
an object.
Length Meter m
• Weight is the force that matter feels due to
Mass Gram g gravity.
• The base unit of mass in the metric system is
Volume Liter L
the gram (g).
Time Second s 1 kilogram (kg) = 1,000 grams (g)
1 kg = 1,000 g
1 milligram (mg) = 0.001 grams (g)
Common Prefixes Used for Metric Units 1 mg = 0.001 g
Prefix Symb Meaning Numerical Scientific
ol Value Notation Measuring Volume
The base unit of volume in the metric system is the
Mega- M Million 1,000,000. 10⁵ liter (L).
Kilo- k Thousand 1,000. 10³
1 kiloliter (kL) = 1,000 liters (L)
Deci- d Tenth 0.1 10⁻¹ 1 kL = 1,000 L
Centi- c Hundredth 0.01 10⁻²
1 milliliter (mL) = 0.001 liters (L)
Mili- m Thousandth 0.001 10⁻³ 1 mL = 0.001 L
Micro- µ Million 0.000 001 10⁻⁶
VOLUME = Length x Width x Height
Nano- n Billionth 0.000 000 001 10⁻⁹ = cm x cm x cm
= cm3
Measuring Length
1 mL = 1 cm3 = 1 cc
The base unit for length is meter (m).
1 meter (m)
English Units and their metric equivalents
1 meter = 0.001 km
1 meter = 100 cm Quantity English Unit Metric-English
Relationship
1 meter = 1000 mm
Length 1 ft = 12 in. 2.54 cm = 1 In.
1 yd =3 ft 1 m = 39.4 In.
1 kilometer (km) 1 mi.= 5,280 ft 1 km = 0.621 mi
1 km = 1,000 m
1 km = 1,000,000 mm Mass 1 lb =16 oz 1 kg = 2.20 lb
1 ton = 2,000 lb 454 g = 1 lb
1 km = 100,000 cm 28.3 g = 1 oz
1 millimeter (mm) Volume 1 qt = 4 cups 946 mL = 1 qt
1 qt = 2 pints 1 L= 1.06qt
1 mm = 0.001 m 1 qt = 32 fl oz 29.6 mL =1 fl oz
1 mm = 0.1 cm 1 gal = 4 qt
Common abbreviations for English units: inch (in.). foot
1 centimeter (cm) (ft). yard (ycl). mile (m1). pound (lb). ounce (oz). gallon
1 cm = 0.01 m (gal). quart (qt) and fluid ounce (I1 oz).
1 cm = 10 mm
Example: how many liters is 1.0 pint of blood?
1 pint x 1qt/2pint x 1L/1.06qt
1 x ½ x 1L/1.06
, Inorganic & Organic Chemistry Reviewer
= 0.472 • Ex: 509 has 3 significant figures.
Significant Figures 3. A final zero or trailing zeros in the decimal portion
✓ An exact number results from counting objects is ONLY are significant.
part of a definition • Ex: .500 or .632000 the zeros are significant
✓ An inexact number results from a measurement or • .006 or .000968 the zeros are NOT significant!
observation and contains some uncertainly
✓ Significant figures are all the digits measured SIGNIFICANT FIGURES IN NUMERICAL
number including one estimate digit COMPUTATIONS
i. Sums and differences - for addition and
Determining the number of Significant subtraction, the result should have the same number
figures of decimal places as the number with the smallest
✓ All nonzero digits are always significant. number of decimal places.
Rules to determine when a zero is a ii. Products and quotients - assume unit uncertainty
significant figure: in the last digit of each number. - the least number of
Rule [1] A zero counts as significant Exa zeroample significant figures in any number of the problem
figure when it occurs: determines the number of significant figures in the
29.05g — four SF
answer.
• Between two non-zero digits
1.0087mL — five SF
• At the end of a number with
25.70 cm — four SF Example: 2.5 x 3.42
a decimal point
3.7500 — five SF - The answer to the problem would be 8.6
620. lb — three SF
- Why? 2.5 has two significant figures while 3.42 has
Rule [2] A zero does not count as a three.
significant figure when it
- Two significant figures is less precise than three, so
occurs:
the answer has two significant figures.
• At the beginning of a number 0.0245 mg — three SF
0.008 mL — one SF
• At the end of a number that
2,570 m — three SF
does not have a decimal point
1,245,500 m — five
SF
RULES FOR DETERMINING THE NUMBER OF
SIGNIFICANT FIGURES
i. Disregard all initial zeros.
ii. Disregard all final zeros unless they follow a
decimal point.
iii. All remaining digits including zeros between
nonzero digits are significant.
THERE ARE THREE RULES ON DETERMINING
HOW MANY SIGNIFICANT FIGURES ARE IN A
NUMBER:
1. Non-zero digits are always significant.
• Ex: 26.38 would have 4 significant figures and 7.94
would have 3.
2. Any zeros between two significant digits are
significant.
