1. Biochemistry Bio= Life Chemistry= science of matter (atoms)
Atomic Structure

2. ATOMS or ELEMENTS
Atoms: are the basic building blocks of matter that make up everyday objects. A desk, the air, even you are made up of atoms!
Matter is anything with mass and volume… so pretty much everything is matter
Mass – how many atoms
Volume – how much space you take up
There are 90 naturally occurring kinds of atoms. Scientists in labs have been able to make about 25 more.
Elements : substance consisting of 1 type of atom

3. History of Atoms… John Dalton (1766-1844)
Dalton was able to perform experiments based off of Democritus ideas and create the atomic theory.

4. Dalton’s Atomic Theory:
All matter is made up of subatomic particles called atoms. (smallest unit of matter)
Atoms of the same element are identical.
Atoms of different elements can physically mix creating a mixture or can chemically combine to form compounds.
Chemical reactions occur when atoms bonds are separated, joined, or rearranged.
However, atoms of one element are never changed into atoms of another element as a result of chemical reaction.

5. smallest unit of matter
All matter is made up of subatomic particles called atoms. (smallest unit of matter)
smallest unit of matter
Living
things
Organ
systems
Organs
Tissues
Together they form
Cells
_____________
__________

6. 2. Atoms of the same element are identical.
Hydrogen atom is = to another hydrogen atom
3. Atoms of different elements can physically mix creating a mixture or can chemically combine to form compounds.

7. Bonds are a result of atoms sharing, taking, or giving up electrons
4. Chemical reactions occur when atoms bonds are separated, joined, or rearranged.
However, atoms of one element are never changed into atoms of another element as a result of chemical reaction.
Bonds are a result of atoms sharing, taking, or giving up electrons

8. Vocabulary you need to know…
Element- smallest unit of matter.
Ex: oxygen, hydrogen
Atom- 1 of the smallest units of matter.
Ex: 1 oxygen, 1 hydrogen
Electrons – Negatively charged subatomic particles, are responsible for all bonding
Protons – Positively charged subatomic particles found in the nucleus of the atom, can be used to
Neutrons – Neutrally or no charged subatomic particle. found in the nucleus of the atom

9. An ATOM… Nucleus = Protons and neutrons
Electrons fly around the nucleus in an electron cloud
The outer most electrons are called valance electrons – they are responsible for all bonding
Mass of the subatomic particles:
Neutron = 1 Proton = Electron =
The mass of the electron is SOOO tiny we don’t even count it when calculating the mass of an atom
Atomic mass = P +N

10. More Vocabulary
Nucleus – The center core of an atom, composed of protons and neutrons.
The nucleus is so dense that if it were the size of a pea it would weigh 250 tons.

11. More Vocabulary
Atomic Number – an element is the number of protons in the nucleus of the atom of that element.
Atomic number = P
Atomic Mass– the total number of protons and neutrons in the nucleus of the atom for all the isotopes of that atom.
Atomic Mass = P + N 5 B
10.81

12. More Vocabulary
Isotopes – atoms that have the same number of protons but a different number of neutrons.
Ions - Atoms that have the same number of protons and neutron but different number of electron which give them a positive (+) or negative (-) charge
When atoms lose an electron it become positive
When atoms gain an electron it become negative

13. Examples of Isotopes
Examples of Ions

14. The number of Protons are what make each element unique!!
example: only oxygen has 8 protons and all oxygen's have 8
Example: only Boron has 5 protons and all boron's have 5

15. B 5 10.81 Anatomy of the Box… Boron Atomic Number Symbol Atomic Mass
Element Name
Atomic Mass B
Boron

16. The atomic number = # protons
To get NEUTRONS you simply subtract the number of protons from the rounded ATOMIC MASS
IF the atom does not have a charge then…
# electrons= # protons
If the atom has a charge (ion) then…
# Electrons = # of protons (+ OR –) the charge
(we will need to flip the charge)

17. Li 3 6.941 Lithium What is the name of this element? Lithium
What is its atomic number? 3
What is its atomic mass?
6.941
How many protons does it have?
How many electrons does it have?
How many neutrons does it have?
6.94 rounded = 7.0
= 4

18. C 6 12.0107 Carbon What is the name of this element?
What is its atomic number?
What is its atomic mass?
How many protons does it have?
How many electrons does it have?
How many neutrons does it have?

19. C 6 +2 12.0107 Carbon What is the name of this element?
6 +2 C
Carbon
What is the name of this element?
What is its atomic number?
What is its atomic mass?
How many protons does it have?
How many electrons does it have?
How many neutrons does it have?

20. Ag 47 +4 107.8682 Silver What is the name of this element? Ag
Silver
What is the name of this element?
What is its atomic number?
What is its atomic mass?
How many protons does it have?
How many electrons does it have?
How many neutrons does it have?

21. O 8 -2 16.0 oxygen What is the name of this element?
16.0 O
oxygen
What is the name of this element?
What is its atomic number?
What is its atomic mass?
How many protons does it have?
How many electrons does it have?
How many neutrons does it have?

22. Atoms to molecules
If you read a book, you will find words on a page. Letters make up those words. In English, we only have twenty-six letters, but we can make thousands of words.
In chemistry, you are working with around 120 elements, and when you combine them you can make millions of molecules.
Molecules are groups of atoms bonded together in the same way that words are groups of letters.
An "A" will always be an "A" no matter what word it’s in. A sodium (Na) atom will always be a sodium atom no matter what compound it’s in.
While the atoms may have different masses and organization, they are all built with the same parts. Electrons, protons, and neutrons make the Universe the way it is.

23. Atoms combine in different ways to form different compounds and mixtures
Atoms are the building blocks of matter

24. To get molecules we need BONDING
Bonding is all about the ELECTRONS
Any type of bonding is considered a chemical change!
There are three main types of bonds
Covalent
Ionic
Hydrogen

25. Covalent Bond
bond in which one or more pairs of electrons are shared by two atoms.
This is a very strong bond!!
Usually occurs between two non metals

27. Polarity – not sharing equally
Polarity occurs when electrons are not equally shared between atoms in a covalent bond.
Polar molecule: Water H20
Non polar molecule N2 N N
Because the oxygen atom is so much bigger then the 2 hydrogen atoms it hogs the electrons
This causes it to have a SLIGHT negative change and the hydrogen to have a SLIGHT positive charge
They are the same size so one can’t bully the other and hog the electrons

28. Bond, Ionic Bond Taken NOT shared
A bond where electrons are given or taken
Usually occurs between a metal and a non metal
This is a medium strength bond but water can easily tear this bond apart
A positive atom is called a cation
A negative atom is called an anion

29. Hydrogen Bond
type of attractive force that exists between two partial electric charges of opposite polarity
Mini opposites attract due to unequal sharing of electrons in covalent bonds
One is not very strong but when there are hundreds this can be a strong bond

30. Combining molecules Two basic ways to combine molecules Compounds
Mixtures

31. Compounds
Compounds are groups of two or more elements that are bonded together.

32. Mixtures
two or more different substances which are mixed but are not combined chemically
Mixtures are absolutely everywhere you look. Most things in nature are mixtures. Look at rocks, the ocean, or even the atmosphere. They are all mixtures, and mixtures are about physical properties, not chemical ones.
Mixture
Compound

34. Physical properties Chemical properties Reactivity Weight
If it burns or not
Acidic or Basic
If it has changed in taste or color- represents a chemical change
Weight
Mass
Volume
Size
Dull
At what temperature does it melt

35. States of matter – Lets get physical
States of matter also called phases are physical changes that happen to elements and molecules.
There are 3 basic phases
Solid
Liquid
Gas

36. Solids are tightly packed and slowest moving with least amount of energy (definite volume and shape)
Liquids flow according to the container have medium movement and energy (definite volume, variable shape)
Gas spreads out as much as it can has the most amount of movement and the most amount of energy (variable volume and shape)

37. As you increase energy you increase temperature which can cause phase changes (these are physical changes)
Endothermic
Adding energy
Removing energy
Exothermic

38. Chemical Vs. Physical changes
Chemical change is any change that involves making or breaking of bonds between atoms. Example:
iron rusting gasoline burning
eggs cooking
bread rising
milk souring
Physical change rearranges molecules but doesn't affect their bonds. Examples:
whipping egg whites (air is forced into the fluid)
boiling water (molecules are still H2O.)
dissolving sugar in water
dicing potatoes (cutting usually separates molecules without changing them.)

39. Question TIME
Describe the differences between the three types of bonds we talked about.
How can you tell a compound apart from a mixture?
Give an example of matter:
Molecules are formed by ____________ bonding together.
What subatomic particle is responsible for all bonding?
If I break a water molecule (H2O) into just Hydrogen and just Oxygen by passing electricity through it, is this a physical change or chemical change?

40. Chemical Reactions
Reactions occur when two or more molecules interact and the molecules change.
 Bonds between atoms are broken and created to form new molecules.
What molecules are they? How do they interact? What happens? The possibilities are infinite. 

41. Energy in Chemical Bonds
Energy is stored in the bonds between atoms.
How about when you burn a piece of wood? When you burn something, you release the energy from the chemical bonds in the wood.
Where did the energy come from? The Sun.
A plant needs the Sun to grow. Light hits the plant and is used by a process called photosynthesis. The plant captures the Sun's energy and stores it in the chemical bonds. You have probably heard of glucose (C6H12O6)
When you burn a piece of wood, you are releasing all of the energy stored up in those chemical bonds. You experience that energy as heat and light (fire). 
Burning it breaks the bonds releasing the energy in the form of light and heat
Stored in plant tissue
Photosynthesis
Energy in bonds

42. Exothermic Vs Endothermic Reactions
Heat is released
Endothermic
Heat is absorbed

43. Demo endergonic and exergonic reactions.+
water +
citric acid
Sodium bicarbonate
citric acid + baking soda (a spoonful of each) + 50 mL of water.
1. What's happening to the temperature?
2. Is this an endothermic or exothermic reaction? How do you know?

44. Calcium Chloride + baking soda + water =
Demo endergonic and exergonic reactions.
Calcium Chloride + baking soda + water =
1. What's happening to the temperature?
2. Is this an endothermic or exothermic reaction? How do you know?

45. The basics of a chemical reaction

46. Practice Identifying parts of a chemical reaction
3 Na + 1 FeBr3  3 NaBr + 1 Fe
Which are the products?
Which are the reactants?
How many Fe in the products side?
How many Fe in the reactions side?