december 12th

December 12thQuick Write:

Take the worksheet at the front of the desk. Work on class work sheet

Homework:• complete the class work sheet on the Periodic Table• Read pages 150-159• write Cornell Notes for pgs 135-149 if not complete

SWBAT:• Explain the difference between a row and a group in the Periodic table.• define the word valence electrons.•Describe each group.

Closure

List the family names.Describe 5 characteristics you learned about

the alkali elements.What do you find in the box of each element?

December 13thQuick Write:

1. Take out your Cornell Notes and the Chart from yesterday.

2. Define valence electron.3. How is the periodic table organized?

Homework:• review your notes• Both Periodic Table Worksheets must be complete by tomorrow (front and back)

SWBAT:• Explain the difference between a row and a group in the Periodic table.• define the word valence electrons.•Describe each group.

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

The Periodic Table

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 Elements1. Metals2. Nonmetals3. Metalloids or

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

4. Noble gases

Metals on the left

Nonmetals on the right

Metalloids semimetals

Group numbers and Family namesWhat are the groups?

The vertical columns Each column is numbered a Group Similar properties but not identical Ex: Group 1: Alkali Metals: Li, Na, K

Soft, white shiny metals All have same number of valence electrons Valence electrons?

The last shell of the atom and the number of electrons

Valence Electron

Periods

Each row is a periodElements are not alike in the propertiesAs you move from left to right the element

goes from an extremely active solid to an inactive gas Why? How can you remember this?

December 14th

Quick Write:1. Place your two Periodic Worksheets on your desk to be

checked for completion.2. Exchange your questions with your partner. Write down

their questions. Class Review

1. What is an ion?

Homework:• study your periodic Worksheets• quiz Friday, December 16th on characteristics of Chemical Families•Test Wednesday, December 21st

Your quizzes will be returned

this week!! : )

SWBAT:• Identify unique characteristics of the Chemical Families.• Differentiate between the traits of each Chemical Family.

December 15th

Quick Write:1. Define ions and valence electrons.

Homework:• study your periodic Worksheets• quiz Monday, December 19th on characteristics of Chemical Families• Test Thursday, December 22nd

Molecular Forces Lab is a week late. Late

labs will lose points / week!

SWBAT:• Identify unique characteristics of the Chemical Families.• Differentiate between the traits of each Chemical Family.

Your quizzes will be returned

this Friday!! : )

Alkali Metals

Description:• Most reactive metals • always found as compounds in nature• 1 valence electron, tend to lose 1 electron to form positive

ions• Family 1

Usage:Sodium: found in table saltRubidium: found in space vehicle engines

Alkaline Earth Metals

Description:• Reactive metals• always found as compounds in nature• 2 valence electrons, lose 2 electron to form positive ions• Family 2

Usage:Strontium (Sr): found in fireworksRadium (Ra): treatment of cancerBarium (Ba): used in glass making

Transition Elements

Description:• hard solids with high melting point• Valence electrons of 1 or 2 and can lose electrons from the next

energy level• Families 3-12

Usage:Silver (Ag) , Gold (Au): JewelryNickel (Ni): coinsZinc (Zn); paint

Boron Family

Description: have 3 valence electrons Boron is a metalloid Other elements below Boron are metals Family 13

Usage:Boron is used to make heat resistant

glasswareAluminum is most abundant metal.

Carbon Family

Description:4 valence electronsContains non-metal, metal and metalloidsFamily 14

Usage:Carbon is known as “the basis of life”Carbon is found in sugars, starches, fats and

proteins

Nitrogen Family

Description:5 valence electronsAtoms share electrons with other atomsFamily 15

Usages:Nitrogen: 78% of the air around usArsenic in insecticides

Oxygen

Description: 6 valence electrons Share electrons when bonding Family 16

Usages:Oxygen: most abundant element in the

Earth’s CrustOxygen: makes up the ozone layer

Halogens

Description:7 valence electronsMost reactive nonmetalsReact with Alkali metals easilyFamily 17

Usages:Chlorine makes table saltFluoride is in toothpaste

Noble Gases

Description:Have 8 valence electronsDo not form bonds with other atomsCalled inert gasesFamily 18

Usages:Radon: cancer treatmentsNeon: produces red light in neon signsHelium fills balloons to float in air, why do they

float?

December 15th

Quick Write:1. Quiz your partner. Write down their questions and then

answer them.

Homework:• study your periodic Worksheets• quiz tomorrow on characteristics of Chemical Families• Test Wednesday, December 21st

Molecular Forces Lab is a week late. Late

labs will lose points / week!

SWBAT:• Identify unique characteristics of the Chemical Families.• Differentiate between the traits of each Chemical Family.

Your quizzes will be returned

this Friday!! : )

Alkali Metals

Description:• ______________________________________________• ______________________________________________• ______________________________________________• _______________________________________________

Usage:________________________________________________________________________

Alkaline Earth Metals

Description:• ______________________________________________• ______________________________________________• ______________________________________________• _______________________________________________

Usage:________________________________________________________________________

Transition Elements

Description:• ______________________________________________• ______________________________________________• ______________________________________________• _______________________________________________

Usage:________________________________________________________________________

Boron Family

Description:• ______________________________________________• ______________________________________________• ______________________________________________• _______________________________________________

Usage:________________________________________________________________________

Carbon Family

Description:• ______________________________________________• ______________________________________________• ______________________________________________• _______________________________________________

Usage:________________________________________________________________________

Nitrogen Family

Description:• ______________________________________________• ______________________________________________• ______________________________________________• _______________________________________________

Usage:________________________________________________________________________

Oxygen

Description:• ______________________________________________• ______________________________________________• ______________________________________________• _______________________________________________

Usage:________________________________________________________________________

Halogens

Description:• ______________________________________________• ______________________________________________• ______________________________________________• _______________________________________________

Usage:________________________________________________________________________

Noble Gases

Description:• ______________________________________________• ______________________________________________• ______________________________________________• _______________________________________________

Usage:________________________________________________________________________

Group Family Name

Description

1 Alkali Metals

• Very reactive metals • always found as compounds in nature• 1 valence electron, lose 1 electron to form

+1 ions2 Alkaline

Earth Metals

• Reactive metals• always found as compounds in nature• 2 valence electrons, lose 2 electron to

form +2 ions3-12 Transition

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

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

18 Noble Gases

• Not reactive, do not form ions• Filled, stable valence shell (8 electrons

except He which has 2)

Group Family Name

Description

13

14

15

16

Rare Earth Metals

What is an ion?

Description of the Periodic TableMetalloids/Semimetals: on the zigzag separates metals from nonmetals Examples: B, Si, Ge, As, Sb, Te, At

Nonmetals: gases, liquids or crystalline solids Examples: 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) Examples: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

Other metals: Z n, 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

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.

Quick Write!1. Atom video

WEDNESDAY, NOVEMBER 23RD

SWBAT:• identify the Atomic Mass and Atomic Number.• Review of the atom and elements

Homework:Enjoy Turkey Day!!!

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.

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)