1. Welcome to Chemistry

2. Chemistry: the study of the composition, structure, and properties
1.1 What is Chemistry?
Chemistry: the study of the composition, structure, and properties
of matter, the processes that matter undergoes, and the energy
changes that accompany these processes
Speaking of which: what are we made of?
Lots of stuff- carbon, oxygen, hydrogen, sulfur, phosphorous, iron, nitrogen,
to name just a few. The human body is composed of many hundreds of millions of
chemical compounds and substances, each just a differing arrangement of elements
from the periodic table.
But where do these things come from?
All of the elements come from the stars, and were made many billions of years ago
through the coagulation of interstellar dust.
How are the elements formed?
In a process called fusion, but we’ll get to that later.
Use kids as matter. Composition – what you’re made of. Hair, eyes, ears, arms, legs, feet… structure- what order is that stuff in. ok its all in the same order but blonde vs brunette..short vs. tall. We’re all made up of the same parts but in different ways (elements). Properties..tall = good at basketball maybe or smart..some could change and some stay the same. Get stronger (lift weights) how much energy are you expending to do so?
What is it made of? How is it put together? How do those things make it unique? How can it change..and at what cost (energy)?

3. Branches of Chemistry
There are several areas of study and research in chemistry which often
overlap with one another. So put on your fun hats, here we go:
1. Organic Chemistry: the study of most carbon-containing compounds
(more on this later as we will begin organic at the end of the year)
2. Inorganic Chemistry: the study of (duh) non-organic substances which have
organic fragments bonded to metals (organometallics)
3. Physical Chemistry; the study of the properties and changes of matter and their
relation to energy.
4. Analytical Chemistry: the ID of the components and compounds of materials.
5. Biochemistry: the study of substances and processes occuring in living things.
6. Theoretical Chemistry: the use of mathematics and computers to understand
the principles behind observed chemical behavior and to design and
predict the behavior of new chemical compounds.

4. Chemistry organic chemistry bio- chemistry inorganic chemistry
physical
chemistry
analytical
chemistry

5. 1.2 Matter and It’s Properties
Matter anything that has mass and takes up space (volume)
and so…
Mass measure of the amount of matter.
Atom: smallest unit of an element that
maintains the chemical identity of
that element.
Examples?
A carbon atom.

6. 1.2 Matter and It’s Properties
Element: a pure substance that cannot be broken down into
simpler, stable substances and is made up of one type
of atom.
Examples?
The element carbon.
For a complete list of elements, where should we look?
More on this later.

7. 1.2 Matter and It’s Properties
Compound: a substance that can be broken down into simple,
stable substances. Each compound is made from atoms
of two or more elements that are chemically bonded.
Examples?

8. 1.2 Matter and It’s Properties
Properties and Changes in Matter
Every substance has characteristic properties.
Properties are either Extensive or Intensive
Extensive Properties:
depend on the amount of matter present.
Examples: mass, volume, amt. of energy
Intensive Properties:
do not depend on the amount of matter present.
Examples: melting point, boiling point, density.

9. 1.2 Matter and It’s Properties
Physical Properties and Physical Changes
Physical Property: a characteristic that can be observed or measured
without changing the identity of the substance.
Examples:
Boiling point (temp. substance goes from liquid to gas)
Melting point (temp. substance goes from solid to liquid)
Freezing point (temp. substance goes from liquid to solid)
Condensation point (temp. substance goes from gas to liquid)
By the way, what is the boiling point of water? Freezing point?
The melting point? Condensation point?

10. 1.2 Matter and It’s Properties
Physical Properties and Physical Changes
Physical Change: a change in substance that does not involve a change in identity of the substance.
Examples:
Grinding, cutting, melting, and boiling a material.

11. Quick Review!
Fill in the blanks with any of the new terms you just learned …
I am an astronaut going to the moon and I’m bringing a scale with me. In space, I will stand on the scale and find that my _______ will be the same but my ______ will have changed.
The graphite in my pencil is only made up of carbon, therefore it is an ________. The rest of my pencil is made up of several things, which makes it more like a _________.
Water always freezes at 0°C. This is a _______ property (hint: there are two correct answers!)
Cutting a piece of paper in half gives me two smaller pieces of paper. Each piece is still has the same chemical characteristics but has less mass. This is called a _______ change.

12. Change of State:
Physical change of substance from one state to another.
Solid: matter in this state has a definite volume and shape.
Liquid: matter in this state has definite volume but indefinite shape.
Gas: matter in this state has neither definite volume or shape.

13. Change of State:
Physical change of substance from one state to another.
An important 4th state of matter is something called
Plasma: high temperature physical state of matter in which atoms
lose most of their electrons.

14. Change of Phase: When a substance goes from one form to
another, (almost) always in the same order.
solid liquid gas
This goes for all substances, remember.
Now, some terms.
HEAT
HEAT
- HEAT
- HEAT

15. Change of Phase (for water):
solid liquid gas
melting/freezing point
boiling/condensation point
0ºC
100ºC
MELTING
BOILING
FREEZING
CONDENSING
(ice)
Think of it like speed..60mph is always 60mph even if I was accelerating or deccerlating
(water)
(steam)

16. 1.2 Matter and It’s Properties
Chemical Properties and Chemical Changes
Chemical Property: a substances ability to undergo changes that
that transform it into different substances.
Examples:
Rusting material-
Iron + Oxygen (g) Iron oxide (rust)
Piece of paper…crumple it, rip it, cut it..still paper. Light it on fire..not paper anymore. (color often a good indicator or chemical change)
(after)
(before)

17. 1.2 Matter and It’s Properties
Chemical Properties and Chemical Changes
Chemical Change: a change in which one or more substances are converted into different substances.
Reactants Products
Reactants: the substances that react in a chemical change
Products: the substances that are formed in a chemical change.
C + O CO2

18. Quick Review!
Fill in the blanks with any of the new terms you just learned …
There are three main phases of matter, they are _____, ______, and ______.
When the ice cube in my drink melts, it is considered a _____________.
I will make Ms. T so proud by NEVER forgetting that the freezing/melting point of water is _____ and the boiling/condensation point is _____.
When iron combines with oxygen, iron oxide, or rust, is produced. This is a ________. Iron’s ability to undergo this reaction is called a _________.

19. Development of the Periodic Table
The modern periodic table of elements is mostly the work of Russian chemist
Dmitri Mendeleev ( ). It was set up in such a way so group elements
in columns according to their properties, but also put them in ascending order
according to their atomic number. Let’s observe:
The vertical columns are called groups; the horizontal rows are called periods.
Periodic Law: when elements are arranged in order of increasing atomic number,
there is a periodic repetition of their physical & chemical properties.

20. Groups The vertical columns are called groups, or families.
There are 18 groups on the periodic table.
Groups

21. The horizontal rows are called periods.
Periodic Law: when elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical & chemical properties.

22. Elements in the same group: physically and chemically similar
Periodic Trends
Elements in the same group: physically and chemically similar
Elements in the same period: ordered in increasing size and atomic number.

23. Metals
Characteristics of metals: excellent conductors of heat and electricity, very reactive, usually make positive ions when dissolved in solution, mix well to make alloys.

24. Group 1A: Li, Na, K, Rb, Cs, Fr. Does not include hydrogen.
Alkali Metals
Group 1A: Li, Na, K, Rb, Cs, Fr. Does not include hydrogen.
▪ They are very reactive because of the lone electron in their outer shell.
▪ Very shiny and light in weight.

25. Alkali Earth Metals Group 2A: Be, Mg, Ca, Sr, Ba, Ra
▪ Not as reactive as alkali metals, but form bonds very easily.

26. are not full. This allows them to bond to many other elements in a
Transition Metals
Have a special electron shell arrangement where two of their outer shells
are not full. This allows them to bond to many other elements in a
variety of shapes.

27. Halogens
Have an outer shell that is almost full, therefore very reactive. Often bond
with metals and elements from group one (alkali metals). When an halogen
combines with another element, the resulting compound is called a halide.

28. Inert Gases (Noble gases)
Include: He, Ne, Ar, Kr, Xe, Rn.
Have a full outer shell and are very unreactive, hence the title “inert”.

29. · Also known as rare-earth or inner-transition elements.
Lanthanide Series
· Also known as rare-earth or inner-transition elements.
· Fifteen elements that start with lanthanum (La) at atomic number 57 and finishing up with lutetium (Lu) at number 71

30. some elements with higher numbers have only been made in labs.
Actinide Series
· These elements are all radioactive and only some are found in nature;
some elements with higher numbers have only been made in labs.
·Fifteen elements that start with actinium (Ac) at atomic number 89 and finishing up with lawrencium (Lr) at number 103

31. Metalloids Metalloids are found on the periodic table
between the metals and non-metals.
Appropriately, they exhibit characteristics of both metals and non-metals.

32. Nonmetals Many nonmetals are gases at room temperature: N; O; F; Cl.
These are elements that are poor conductors of heat and electricity.