1. Friday 10/14/16 AIM: How are all living things built?
DO NOW: In your own words, explain what you have in common with a rock
Homework:text read pages answer question
1-3 page 54

2. Chemistry
The Study of Matter

3. Living vs nonliving things
Living things display all characteristics of life whereas nonliving things display some but not all characteristics of life
Both living and nonliving things are made up of atoms
Atom: basic building block of all matter
Matter: anything that has mass and takes up space:
EX: the gases that make up the air, the desk, you , the cells that make you, water etc.

4. Matter Anything that has mass and takes up space
Ex: The human body, the air and atmosphere surrounding us, the Atlantic ocean
Found on earth in 3 states
Solid, liquid, gas
The state or phase of matter is determined by the atomic arrangement

5. States of Matter Rap - YouTube

6. Properties of matter
Directly related to arrangement of atoms

7. Three Classes of Matter
1. Elements
the most basic types of matter
2. Compounds
2 or more elements bonded together in
definite proportion
3. Mixtures
two or more substances (elements and or compounds) physically combined, but
not chemically bonded

8. Elements Substances that are made up of all of the same type of atom
They cannot be broken down into anything else
Periodic table of elements that lists all known elements with their symbols and properties
Each element has its own unique properties
EX: boiling point, freezing point, melting point, reactivity rate
Once you change the structure of an atom, you change the element that it builds!!!!!!!!!!!!!!!!

9. Elements
basic types of matter that can not ordinarily be broken down into simpler substances
How many are found in nature? 92
Which ones are normally present in humans ? 26

10. Important Elements In Organisms
Hydrogen (H) Oxygen (O)
Carbon (C) Nitrogen (N)
Calcium (Ca) Phosphorous (P)
Potassium (K) Sulfur (S)
Sodium (Na) Chlorine (Cl)
Magnesium (Mg) Iodine (I)
Iron (Fe) others = 0.1%
96% of your body mass is made up of : CHON
O (65%) + C (18%) + H (10%) + N (3%)

11. Examples of Elements: Periodic Table

12. Living things are made up of elements
CHNOPS: major elements that build living things
All other elements are found in small amounts so they are called trace elements

13. All matter is built from atoms
Atom is the basic unit of matter
Subatomic particles
Nucleus
Protons
Neutron
Orbiltals
Electrons

14. Atoms the smallest particles of an element
contain protons, electrons and neutrons
1. Protons:
charge = +1
location: in nucleus (center) of atom
Give some of the atomic mass
Identified by the atomic #

15. 2. Electrons:
charge = -1
location = orbiting outside the nucleus
Insignificant mass
React with electrons of other atoms to form bonds
3. Neutrons
charge = 0
location = in nucleus (center) of atom
Help to give atomic mass

16. The Structure of an Atom

17. How are subatomic particles arranged?
CHE1.3-e-Animation table for the first 11 elements of the Periodic Table

18. Properties of Atoms 1. Electrically neutral total charge = 0, because:
# electrons = # protons
2. Atomic Number
refers to the number of protons in the nucleus of the atom
determines behavior & type of element
3. Atomic Mass Number
# of protons + # of neutrons
IF YOU CHANGE THE # of protons or neutrons, you change the element that the atom builds!!!!

19. How do we build bigger molecules and compounds from atoms?
Through electron bonding
Electrons may be gained, lost or shared between atoms to build larger molecules and compounds

20. What is the atomic # of carbon?
What is the atomic mass number of oxygen?
What would happen to the electrical charge of these atoms if an electron were removed? Gained?

21. Why is it important for an atom to be able to gain or lose electrons?
ANSWER: Because loss or gain of electrons is one way we can build a bond!!!!

22. How is an atom effected if the atomic number changes?

23. What would happen to an atom if we added an electron?
The atom becomes negatively charged.

24. Ion Charged atom That means electrons have been added OR
Gives the atom (-) charge OR
Electrons have been removed
Gives the atom (+) charge

25. What happens if I change the number of electrons in an atom?
Create an ion: charged atom

26. How is an atom affected if the number of neutrons is changed?

27. Atomic Mass would change
Explain what would happen to an atom if the number of neutrons changed.
Atomic Mass would change

28. Aim: Why is water important to living things?
DO NOW: What is an ion? And how are ions formed?
HW: Textbook read pages answer questions 1-3 on page 48
WRITE OUT QUESTION AND ANSWER

29. Forces That Hold Atoms Together
Electrical Force
opposite charges attract
electrons (-) orbit around nucleus because the nucleus is positive (+)
Nuclear Force
holds the protons and neutrons together within the nucleus

30. Using the periodic table of elements
Each element has a specific number of protons, neutrons and electrons
You can look up an element to get the number of protons, neutrons and electrons
Atomic number- # protons in the nucleus
Atomic mass- # protons + # neutrons in the nucleus

32. If an atom has an atomic number of 6 and an atomic mass of 12
How many electrons are found in its orbitals?
What would happen to the charge of the atom if it gains an electron?

33. Carbon

34. Carbon (C)
Atomic number 6
Atomic mass 12
# p=6
#n=6
#e-=6

35. Properties of Carbon
Capable of sharing 4 electrons with 4 different atoms
Forms 4 covalent bonds
This gives carbon the ability to build all of the molecules and compounds that help to build you

36. Organic chemistry
The branch of science dealing only with the study of molecules and compounds built from Carbon atoms

37. Importance of bonds
Atomic forces and properties along with electron interactions help atoms to form bonds
Bonds between atoms build molecules and compounds
Molecules and compounds build cells
CELLS BUILD YOU!!!!!!!!!!!!!!!!

38. Ionic and covalent bonding animation - YouTube

39. Chemical Bonds 1. Ionic Bonds bind atoms together
involve sharing or transfer of electrons
Two basic types of chemical bonds
1. Ionic Bonds
electrons are transferred from one atom to another
creates charged particles called ions
when atoms lose electrons they become:
positive ions
negative ions are produced when atoms:
gain electrons
Opposite charges attract forming a bond

40. Ionic Bond (NaCl)

41. 2. Covalent Bonds electrons are shared by two different atoms
electrons will now orbit around both nuclei
produce “molecules”
a molecule is a distinct group of two or more atoms held together by covalent bonds

42. Covalent Bonding

43. Atomic bonding

44. Ionic vs. Covalent Bonds

45. Compounds Two or more elements joined together by chemical bonds
The properties of a compound are very different from the properties of the individual elements it contains
The smallest unit of a covalently bonded compound is a molecule

46. Water: a polar molecule
electrons are shared unequally between H & O
Oxygen tends to be an electron fiend and likes to steal electrons from other atoms
shared electrons are more attracted to:_____
Answer: oxygen
A water molecule is constantly losing and gaining hydrogen ions that is what give it unique properties

47. Example of Hydrogen Bonds

48. Properties of water
Water is unique in that it is the only natural substance that is found in all three states -- liquid, solid (ice), and gas (steam) -- at the temperatures normally found on Earth.
Water is called the "universal solvent" because it dissolves more substances than any other liquid.
Water has a high solubility for many solutes

49. Making solutions
basically two substances that are physically combined but not chemically bonded.
One of them is called the solute. A solute is the substance to be dissolved (sugar).
The other is a solvent. The solvent is the one doing the dissolving (water).
Solubility: the ability of the solvent to dissolve the solute

50. Solutions
Solute and solution will combine until all molecules are saturated
At this point solute will sink to the bottom
EX: when you put too much ice tea mix in water all the sugar falls to the bottom

51. Examples of Elements: Periodic Table

52. Acids, Bases and Neutral Solutions

53. Ionization of Water
ionization means the release of ions (charged particles) from a compound
H+ is a “hydrogen ion”, it was a hydrogen atom
before it lost an electron
OH- is a “hydroxide ion”, it gained an extra election when H+ was released from water
Pure water is a neutral solution because the number of H+ is equal to the number of OH-

54. Acids Compounds that release hydrogen ions (H+)
when they are added to water
Examples: (don’t memorize)
1. Hydrochloric acid (HCl)
HCl  H+ and Cl-
2. Carbonic acid: (H2CO3)
H2CO3  H+ and HCO3-
3. Nitric acid: (HNO3)
HNO3  H+ and NO3-

55. Bases (alkali) compounds that absorb hydrogen ions or
release hydroxide ions (OHֿ)
Examples: (don’t memorize)
1. Sodium hydroxide (NaOH):
NaOH  Na+ and OH-
2. Potassium hydroxide (KOH)
KOH  K+ and OH-

56. Acidic, Basic & Neutral Solutions
Acidic solution:
H+ > OH-
Basic solution:
H+ < OH-
Neutral solution:
H+ = OH-

57. Acid Base Indicators 1. Red Litmus Paper
indicates bases by turning blue
2. Blue Litmus Paper
indicates acids by turning red
3. Bromothymol
yellow in acids, green near neutral and blue in bases
4. pH paper
turns various colors to indicate acids, neutral solutions and bases
can also indicate the strength of an acid or
base

58. Acid-Base Indicators

59. pH scale - based on the concentration of hydrogen ions in a solution
- used to indicate the strength of acids and bases
- ranges from 0 to 14
- acids have pH’s < 7, bases have pH’s > 7
- neutral solutions have a pH of 7
- the farther from 7 the greater the strength of the acid or base
based on powers of 10
- each decrease of 1 digit on the pH scale means 10 times as many hydrogen ions

61. Questions about pH
How would you describe solutions with the following pH’s? 2? 8? 6? 13? 7?
As pH increases, H+ concentration _____
As pH decreases, acidity ________
The H+ concentration in a pH of :
2 is _____________greater than a pH of 4
3 is _____________greater than a pH of 7
1 is _____________greater than a pH of 4

62. AIM: Why is carbon such a vital element to living things?
DO NOW: Look through yesterdays notes and explain how water is built and why it has a partial charge.
What does the word vital mean?
Homework: Project # 2 due Friday

63. AIM: How do atoms combine to build large molecules and compounds?
DO NOW: Explain the structure of an atom
List the 6 elements found in the largest amount in a living thing
HW: Text reread pages Answer questions 2,3,4 pg 54