Quick Write!1. Quiz!

WEDNESDAY, NOVEMBER 16TH

SWBAT:• describe the following and provide examples:• Chemical formula• Chemical equation

• describe the parts of an atom and draw an image • label the subatomic particles• compare and contrast between compounds and elements

Homework:• read workbook pgs 15-23• complete all pages due Friday!• find 10 chemical elements that can be found in your house by Friday•Test Tuesday 11/22

AN ATOM

Basic unit of matter, “unable to be cut”

An Element Pure substance entirely of one atom

WHAT ARE THE SUBATOMIC PARTICLES? Proton Neutron Electron

THE ATOM

Nucleus

(a) (b)

Cloud of negativecharge (2 electrons)

Electrons

WHO IS NEILS BOHR?

He proposed a theory: an atom is composed of a dense

nucleus with electrons in its surrounding orbit

electrons must have a certain amount of energy to orbit the nucleus.

Electrons have a more fixed manner around the nucleus.

MODERN ATOM MODEL Electron cloud model Protons

Have a positive charge have a mass of 1.67 x 10-24 g

Atomic number: number of protons

Electrons: Have a negative charge If the atom has no charge there are the same

number of electrons to protons

Mass number: sum of the protons and neutrons together

Quick Write!1. Take out your sheet

from yesterday.

THURSDAY, NOVEMBER 17TH

SWBAT:• describe the following and provide examples:• Chemical formula• Chemical equation

• describe the parts of an atom and draw an image • label the subatomic particles• compare and contrast between compounds and elements• Calculate the number of neutrons, protons and electrons

Homework:• read textbook pgs. 99 -104 see website for details• read workbook pgs 15-23• complete all pages due Friday!• find 10 chemical elements that can be found in your house by Friday•Test Tuesday 11/22

Quick Write!1. Take out your sheet

from yesterday.2. Answer the Quick

Write Questions

FRIDAY, NOVEMBER 18TH

SWBAT:• describe the following and provide examples:• Chemical formula• Chemical equation

• describe the parts of an atom and draw an image • label the subatomic particles• compare and contrast between compounds and molecules• Calculate the number of atoms found in each chemical formula

Homework:•Test Tuesday 11/22 Read pgs. 120- 126 practice note taking as you did last night

QUICK WRITE1. List the subatomic particles. Proton Neutron Electron2. Where are each of the particles found and

what is their charge? Proton : + charge , found in nucleus Neutron: no charge, found in nucleus Electron: - charge, found outside of the

nucleus

3. Identify one difference between a molecule and a compound.

Molecules are made of atoms, and compounds are made up of molecules, Label the molecule and the compound: ______________C2H4O2

______________H2O

4. What does a chemical formula tell you? A chemical formula tells you the elements

and number of atoms that are needed to make the molecule or compound.

5. What does a chemical equation tell you? A chemical equation tells you the types of

molecules and or compounds that are needed to complete a chemical reaction to form products.

6. What is a subscript? They are found to the lower right of

each element’s symbol. Provides you the number of atoms of

the element in the compound or molecule.

7. What does the coefficient tell you? Tells you the number of molecules and

atoms found in each chemical equation

NOW LET’S HAVE SOME PRACTICE!

Quick Write!1. Place your

homework on your desk.

2. Complete last week’s worksheet

MONDAY, NOVEMBER 21ST

SWBAT:• identify the Atomic Mass and Atomic Number.• compare a solution to a compound.• compare a heterogeneous mixture to a homogeneous mixture.

Homework:Study for Test see website for details.

ATOMIC STRUCTURE

15 7N

Mass Number = protons + neutrons How can you identify it? It is the larger number. It is the mass of the nucleus. Why? Because it contains the protons +

neutrons.

Atomic number = number of protons Smaller number When an atom has no charge, the protons

and electrons are equal in number! Used to identify the element

Atomic number equals the number of ____________ or ________________.

Mass Number equals the number of ______________ + _______________.

The Atom

Atomic NumberSymbolNameMass Number

protonselectrons

protonsneutrons

II. PERIODIC TABLE

CLOSURE Answer the following:

1. What is the difference between a heterogeneous and homogeneous mixture? The heterogeneous mixture will separate upon

standing, you can still see the individual particles and it is not uniform throughout.

A homogeneous mixture is uniform throughout, will not separate upon standing and you cannot see individual particles.

2. What is the difference between a compound and a solution?

A compound must be separated by chemical means and a solution can be separated by physical means.

SOLVING FOR THE NUMBER OF NEUTRONS

Number of neutrons = mass # - atomic #

Question: If the mass number is 15, there is no charge on the atom and the atomic number is 7. How many electrons and neutrons do you have?

Assignment: Finish the rest of the worksheet and turn it in to your teacher.

ATOM ACTIVITY

Name__________________________ Date ______________

WHAT IS AN ATOM?DESCRIBE THE SUBPARTS OF THE ATOM:

DRAW AND LABEL AN ATOM

COMPARE AND CONTRAST BETWEEN A COMPOUND AND MOLECULE

EXPLAIN AND PROVIDE 3 EXAMPLES FOR EACH

CHEMICAL FORMULAS CHEMICAL EQUATIONS

Element Atomic #

Atomic Mass

Mass Number

Protons Neutrons Electrons

1.

2.

3.

4.

5.

6.

7.

EACH ELECTRON IN AN ATOM HAS ITS OWN DISTINCT AMOUNT OF ENERGY.

When electrons are in their lowest energy state, it is called the ground state

The ground state for Na is 2-8-1

elements: Periodic Table are arranged in increasing atomic number.

Placement or location of elements on the Periodic Table indicates the physical and chemical properties of that element.

Number of protons in an atom (atomic number) identifies the element

Atomic mass: found on the Periodic Table of the Elements

CLASSIFYING ELEMENTS Metals Nonmetals metalloids or

semimetals (B, Si, Ge, As, Sb, Te),

noble gases

Metals on the left

Nonmetals on the right

Metalloids semimetals

GROUP NUMBERS AND FAMILY NAMES Group 1 Alkali Metals

Very reactive metals, always found as compounds in nature

1 valence electron - lose 1 electron to form +1 ions

Group 2 Alkaline Earth Metals Reactive metals, always found as compounds in

nature 2 valence electrons - lose 2 electron to form +2 ions

Group 17 Halogens Reactive nonmetals 7 valence electrons - gain 1 electron to form –1 ions

Groups 18 Noble Gases Not reactive – do not form ions Filled, stable valence shell (8 electrons except He

which has 2)

CLASSIFICATION OF THE ELEMENTS Groups 3 - 11 Transition elements:

an element in a transition, hard solids with high melting point, half filled orbitals, far less reactive than Group 1 & 2

Metalloids/Semimetals: on the zigzag separates metals from nonmetals B, Si, Ge, As, Sb, Te, At

Nonmetals: gases, liquids or crystalline solids C, N, O, F, P, Br, gain electrons to become – ion, poor conductors of heat and electricity

Other metals: metals good conductors of heat and electricity, luster and shine, malleable (can change shape) Zn, Hg, Sn, Bi, Po

COMPARING THE PHYSICAL PROPERTIES OF METALS AND NONMETALS

Silvery gray color except copper and gold

Solid at room temperature except mercury

Good conductors of heat and electricity

Malleable – can be hammered into shapes (thin sheets)

Ductile – can be pulled into wires

Many different colors Sulfur – yellow Chlorine – green Bromine – orange Iodine - purple

Many different states (phases) H, N, O – gas Br – liquid S, C, I – solid

Poor conductors of heat and electricity (except carbon)

Brittle – breaks when hit

Metals Nonmetals

FIND THE NAME OF EACH SYMBOL

Group 1 Alkali metals: Li, Na, K, Rb, Cs, Fr Group 2 Alkaline earth metals: Be, Mg, Ca,

Sr, Ba, Ra Transition elements: groups 3 - 11 Other metals: Zn, Hg, Sn, Bi, Po Semimetals: B, Si, Ge, As, Sb, Te, At Nonmetals: C, N, O, F, P, Br Group 18 Noble gases: He, Ne, Ar, Kr, Xe,

Rn

ALL ELEMENTS ARE SOLID AT ROOM TEMPERATURE EXCEPT FOR THE FOLLOWING:

Liquids Mercury (Hg) - the

only liquid metal at room temperature

Bromine (Br) - the only liquid nonmetal at room temperature

Gases Hydrogen (H) Oxygen (O) Nitrogen (N) Fluorine (F) Chlorine (Cl) All of group 18 (noble

gases)Helium (He), Neon (Ne) Argon (Ar), Krypton (Kr), Xenon (Xe), Radon (Rn)