• AIM: How are all living things built?

• DO NOW: In your own words, explain how your body is built.

• Homework:text read pages 51-53. answer the reading check questions on pages

51 and 52. answer question 1 page 54

Tuesday 10/29/13

• AIM: How are living things built?

• DO NOW: What is matter

• HOMEWORK: pg 54 q 2

Chemistry

The Study of Matter

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

States of Matter Rap - YouTube

Properties of matter

• Directly related to arrangement of atoms

Classes of Matter1. Elements

the most basic types of matter2. Compounds

2 or more elements covalently bonded together in definite proportion

3. Mixturestwo or more substances (elements and

or compounds) physically combined, but not chemically bonded

Elements can combine to form molecules and compounds

• Molecule: combination of at least 2 atoms – Can be atoms of the same

type or of different types

– Ex: O2

• Compound: two or more different elements chemically bonded together through electron interaction

Compounds

• The properties of a compound are very different from the properties of the individual elements it contains

• The ratio of elements within a compound is fixed and is indicated by it’s chemical formula

Take out a clean sheet of paper

• Place your heading on top

• Explain what matter is and give an example of matter

Elements• basic types of matter that can not ordinarily be

broken down into simpler substances

• Each element is built from only one type of atom

• How many are found in nature?

92• Which ones are normally present in humans?

26

Examples of Elements: Periodic Table

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) 13 others = 0.1%

• 96% of your body mass is made up of : CHON• O (65%) + C (18%) + H (10%) + N (3%)

10/30/13

• Aim: How does the structure of an atom give it its properties?

• DO NOW: Explain the difference between atomic arrangement in a solid, liquid and gas

• HW: Text read pages 52-53. Question 2 page 54. Explain the importance of valence electrons.

All matter is built from atoms• Atom is the basic unit of matter

– Subatomic particles• Nucleus

– Protons

– Neutron

• Orbiltals– Electrons

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 #

Examples of Elements: Periodic Table

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

The Structure of an Atom

Properties of Atoms1. Electrically neutral• total charge = 0, because:

# electrons = # protons2. Atomic Number• refers to the number of protons in the

nucleus of the atom

• determines behavior & type of element3. Atomic Mass Number

# of protons + # of neutrons

Examples of Elements: Periodic Table

Finding the Contents of an Atom from Atomic # & Atomic

Mass #• # of protons =

atomic number

• # of electrons = atomic number

• # of neutrons = atomic mass # - atomic number

Van der Waal’s Forces 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• overcomes repulsion of + charged

protons

• What is the atomic # of phosphourous?

• What is the atomic mass number of oxygen?

• What would happen to the electrical charge of these atoms if an electron were removed?

• AIM: How does the structure of an atom give the atom its properties?

• DO NOW: Atomically speaking, why are platinum and gold different metals?

Homework: Textbook page 155 questions 4-6

DO NOT FORGET TO WRITE OUT THE QUESTION FOLLOWED BY THE ANSWER

Thursday 10/31/13

• AIM: How do atoms act when the subatomic particles change?

• DO NOW: Explain the importance of the atomic number and the atomic mass. (What information about the atom can you get?)HOMEWORK: Be safe

Thursday 10/31/13

• Atomic #: • Atomic mass:• # p• #n• #e-

108

How are subatomic particles arranged?

CHE1.3-e-Animation table for the first 11 elements of the Periodic Table

1- If I change the atomic number of an atom, what happens to that atom?

2- If I change the number of electrons in an atom, what happens to the atom?

3- # P

# N

# e-

ion_Li

Isotopes• atoms with the same atomic number but different

atomic masses

• atoms of the same element with different numbers of neutrons

• isotopes of oxygen (atomic number = 8)

• O – 16 contains: 8 protons, 8 electrons, 8 neutrons

• O – 18 contains: 8 protons, 8 electrons, 10 neutrons

Isotopes

• Hydrogen Atomic Mass = 1

Atomic Number = 1

• Deuterium  Atomic Mass = 2 

Atomic Number = 1

Uses for Isotopes• Researchers use isotopes as “tracers” to distinguish

between different sources of the same element

Example:• In photosynthesis:

carbon dioxide & water glucose & oxygen gas

• If plant receives carbon dioxide with O-16 and water with O-18, it will release molecules of oxygen gas containing 0-18

• Conclusion:The oxygen gas comes from water molecules not

carbon dioxide

Radioisotopes• contain so many neutrons that they are unstable

• release particles or “radiation” and are called “radioactive”

• can be damaging to cells

• lose their radioactivity at a fixed rate

• the “half life” of a radioisotope is the amount of time it takes for 50% of the atoms to lose their radioactivity

• location can be easily detected and visualized because of their radioactivity

Radioactive isotopes

• They break down at specific rates

• Half life: the amount of time it takes for half of the isotope to break down

• Scientists determine the age of fossils by measuring how much radioactive decay is left

How can these isotopes be useful?

Uses for Radioisotopes• Used to:

• kill cancer cells

• “trace” atoms from one compound to another within organisms

(Carbon-14 is frequently used this way)

• visualize internal organs

• find the age of fossils and other materials

Images of the Thyroid Gland Using Radioactive Iodine

Explain the difference between an ion and an isotope

Friday 11/1/13

• AIM: How do the properties of an atom effect it’s reactivity?

• DO NOW: How is an atom effected if you change the number of neutrons? Electrons?

• Homework: internet project

How is an atom effected if the atomic number changes?

What would happen to an atom if we added an electron?

The atom becomes negatively charged.

Ion• Charged atom

• That means electrons have been added– Gives the atom (-) charge

• OR

• Electrons have been removed– Gives the atom (+) charge

What happens if I change the number of electrons in an atom?

Create an ion: charged atom

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

Explain what would happen to an atom if the number of neutrons

changed.Atomic Mass would change

List and give a brief function of each subatomic particle

Wednesday 11/6/13

• AIM how do atoms combine to form bonds?

• DO NOW: explain the structure of an atom

• HOMEWORK: Handout 6.1

How are rocks similar to coral?

How do atoms build rocks and coral

Ionic and covalent bonding animation - YouTube

Chemical Bonds• bind atoms together• involve sharing or transfer of electrons between two

atoms

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

Ionic Bond (NaCl)

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

Covalent Bonding

Atomic bonding

Ionic vs. Covalent Bonds

Write at least one complete sentence explaining the

difference between an ionic and covalent bond

Friday 11/8/13

• AIM: How does the atomic bonding of water give it unique properties?

• DO NOW: Explain the difference between an ionic and covalent bond

• Homework: Project due Wednesday 11/13/13

• I am aware that I have an internet project due Wednesday 11/13/13. If I do not hand it in on time I will have 3 detentions

Water: a polar molecule• electrons are shared unequally between H & O• Oxygen is an electron fiend!!!!!!!!!

– It will pull electrons closer to its nucleus during a covalent bond creating partial charges

• The area of the molecule containing oxygen will be __________, while the areas containing hydrogen will be ___________

Answers: negative, positive

What causes water molecules to stick to each other?

– Shockwave

• Shockwave

Water is the universal solvent

• Capable of dissolving a wide range of substances

• Due to it’s polarity (partial charge)

• Positive and negative poles are attracted to oppositely charged regions of dissolving molecules

• dissolve

Unique properties allow for cohesion

• Hydrogen bonding causes water molecules to stick together

• Cohesion: tendency of water molecules to resist breaking

Water

• Adhesion: tendency of water molecules to stick to surfaces

• Helps water molecules to move between thin tubes and small spaces

• Cohesion along with adhesion, allow for meniscus formation and capillary action

Tuesday 11/12/13

• AIM: How can you determine the pH of a solution?

• DO NOW: List the parts of an atom and give a brief description of its function

• Homework: Internet project

Examples of Elements: Periodic Table

What does it mean for water to be polar?

Partial charge due to unequal sharing of electrons in a covalent bond

Ionization of Water• ionization means the release of ions (charged

particles) from a compound

H2O H+ and OH-

• H+ is a “hydrogen ion”, it was a hydrogen atom before it lost an electron

• OH- is a “hydroxide ion”, it gained an extra electron when H+ was released from water

• Pure water is a neutral solution because the number of H+ is equal to the number of -OH

Acids, Bases and Neutral Solutions

AcidsCompounds 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-

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-

Acidic, Basic & Neutral Solutions

• Acidic solution:

H+ > OH-

• Basic solution:

H+ < OH-

• Neutral solution:

H+ = OH-

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

pH, the power of hydrogen

In your own words explain the ionization water

Thursday 10/22/09

• AIM: How do we determine the acidity or alkalinity of a solution

• DO NOW: Explain the difference between an acid and a base.

• Homework: Practice exam questions

• pH= percent hydrogen– Measures the amount of H+ ions in a solution

• How would you describe solutions with the following pH’s? 2? 8? 6? 13? 7?

• As pH increases, H+ concentration _____

• As pH decreases, acidity ________

Acid Base Indicators1. Red Litmus Paper

indicates bases by turning blue

2. Blue Litmus Paperindicates acids by turning red

3. pH paper• turns various colors to indicate acids,

neutral solutions and bases

• can also indicate the strength of an acid or base

Red in acid blue in base4. Bromothymol

yellow in acids, green near neutral and blue in bases

Acid-Base Indicators

Mixtures• Two or more substances that are physically combined,

but not chemically bonded

• Each substance keeps it’s own characteristics

Mixtures with an even distribution of substances arecalled solutions

In a liquid solution: -the liquid that makes up most of the solution is

the solvent

-substances that dissolve in the solvent are solutes

Chemical Reactions• Involve the formation and/or breakdown of

chemical bonds

• Produce new substances that were not present before the reaction

• Either absorb or release energy

• Law of Conservation of Matter

matter cannot be created or destroyed in a

chemical reaction

Chemical EquationsSymbolize the effects of chemical reactions

Example: H20 + CO2 H2CO3

Reactants:

• substances present before the reaction

• written before the arrow (H20 + CO2)

Products:

• new substances produced by the reaction

• written after the arrow (H2CO3)

Equations must be “balanced”

1. _________________What is the atomic number of the nitrogen atom? - --------

2. _________________What is the atomic mass of nitrogen? ----------------------

3. _________________What are 2 or more substances that are physically combined

but not chemically bonded?

4. _________________What are atoms of the same element that have a different number of neutrons?

5. _________________Two or more elements that are chemically combined in a definite proportion are known as __________.

6. _________________What type of bond occurs when electrons are transferred?

7. _________________What type of bond occurs when there is unequal sharing of

electrons?

8. _________________Charged particles are known as _______.

9. _________________ Name one use for a radioisotope.

10. _________________What would make an atom electrically neutral?