Hunnicutt Unit 2: Atoms and Elements 1Unit 2: Atoms, Elements, and Bonds

This unit we will talk about:1. Lesson 1: Atoms

a. What makes up an atom?b. What is the function of an atom?

2. Lesson 2: Elementsa. How are Elements organized?b. What is an element?c. Why are elements important?d. What is the Periodic table?e. How do elements bond with each other?

3. Lesson 3: Classifying Mattera. We will discuss the different states of matter

4. Lesson 4: Covalent and Ionic Bondsa. What do elements form compounds?b. How are compounds formed?c. Compare and contrast covalent and ionic bonds

Unit 2 Test: _________________________________________________________

Hunnicutt Unit 2: Atoms and Elements 2Check List of Assignments

Note Packet Vocabulary Workbook

o Chapter 1 Lesson 3 o Chapter 2 Lesson 1 and Lesson 2o Chapter 3 Lesson 2 and 3

Unit KWL Chart Rock Candy Lab (depending on behavior) Atomic Theory Time Line Atom Builder Introduction to Atoms Quiz Elements Quiz Build an Atom Periodic Table Scavenger Hunt Mystery Monday Labs

Matter Quiz Matter Worksheet Ionic and Covalent Bonds Quiz Edpuzzel Review

o Atomic Theoryo Elementso Periodic Tableo Ionic and covalent Bonds

Review Quizizzo Atomic Theoryo Elementso Periodic Tableo Ionic and Covalent Bonds

Unit 1 Test

Unit 2 TimelineDay 1: Atomic Model

History of the Atomic TheoryDay 2: Parts of an AtomDay 3: Mystery MondayDay 4: Atom Quiz/Organizing ElementsDay 5: What is an ElementDay 6: Elements Quiz/Build an ElementDay 7: Periodic Table Scavenger Hunt Day 8: Rock County LabDay 9: Classifying Matter

Day 10: Types of MixturesDay 11: Matter Quiz/Matter WorksheetDay 12: Mystery FridaysDay 13: Mystery MondayDay 14: Ionic Bonds/Ionic Bonds WorksheetDay 15: Covalent Bonds/covalent Bond WorksheetDay 16: Ionic Bonds and Covalent Bonds QuizDay 17: Edpuzzel Reviews (will need headphones)Day 18: Review DayDay 19: Unit 2 Test

Hunnicutt Unit 2: Atoms and Elements 3Vocabulary List (Due on the day of the test)Directions: Look up the definition of the term in your workbooks. Write the definition. Use the word in a sentence.

1. Atom2. Neutron3. Electron 4. Nucleus5. Proton6. Energy level7. Atomic number8. Isotopes9. Mass number10. Atomic mass11. Periodic table12. Chemical symbol13. Period14. Group 15. Valence electrons16. Chemical bonds17. Elements18. Molecule19. Compound20. Chemical formula21. Mixture22. Ion23. Ionic bond24. Ionic compound25. Covalent bond26. Double bond27. Triple bond28. Molecular compound 29. Nonpolar bond30. Polar bond

Hunnicutt Unit 2: Atoms and Elements 4Lesson 1: Structure of Atoms

The Beginning• 430 BC _________________________ proposed that

• “matter was made of small pieces that couldn’t be cut”

• Coined the term __________________________________

• 1800’s ______________________________ Atomic Theory

• Smooth hard balls that _______________________________ be broken down any smaller

Atomic Theories • Thomson’s model (1897)

• Atoms are made of _______________________ parts

• (Dalton didn’t get it quiet right)

• Discovered ______________________ charged particles

• Called them ___________________________!

• Couldn’t figure out what was in the middle

• Assumed it had to be _______________________ charges

• An atom is like a watermelon full of seed (electron)

• Rutherford's Model (1911)• Oh no he challenged his teacher!

• Let see what happens when I shoot stuff a gold (pic next slide)

• Mostly _____________________ space except in the middle

• The __________________________ must be positive because like repels like.

• Nucleus _________________________________________________________________

• The nucleus is made of what would later be called ____________________________________

• Bohr’s Model (1913)• ___________________________________ are found in orbits not random

• Look like ___________________________ moving around the sun

Hunnicutt Unit 2: Atoms and Elements 5

• Cloud Model (1920’s)• Next to last 1

• Electrons _________________________________ orbit the nucleus like planets

• Move _____________________________ within a cloudlike region around the nucleus

• Electrons movement is related to its ____________________________________ level

• James Chadwick (1932)• __________________________ something else in nucleus

• Discovered the ______________________________

• ________________________________________________________________________

• Nucleus has both ________________________ (positive) and _____________________

(neutral)

• Most of the volume is made of __________________________

Day 1 Review

Hunnicutt Unit 2: Atoms and Elements 6

Theories Date Discovery/Description of Model

Day 2 Atoms are ___________________________________________________________________________ Atoms are made of 3 types of particles list them below.

1) __________________ and they are ______________________

2) __________________ and they are ______________________

3) __________________ and they are ______________________

Protons• ________________________________________

• Help make up the nucleus of the atom

• Help _____________________ the atom (could be considered an atom’s DNA)

• _____________________ to the atomic number of the atom

• _________________________ to the atomic mass

• ________________________ to the number of electrons

Neutrons

Hunnicutt Unit 2: Atoms and Elements 7• _____________________________ particles; have no electric charge

• Help make up the ________________________ of the atom

• _____________________________ to the atomic mass

Electrons• ________________________________ charged particles

• Found ____________________________ the nucleus of the atom, in the electron

__________________/levels; each orbit/level can hold a maximum number of electrons (1st = 2, 2nd = 8,

3rd = 8 or 18, etc…)

• Move so ___________________________ around the nucleus that they create an electron cloud

• Mass is ____________________________ when compared to protons and neutrons

• ___________________________ to the number of protons

• Involved in the __________________________ of chemical bonds

Brain Brake

Proton Neutron Electron

Function

Charge

Location in the Atom

Weight

Label and Atom

Atomic Number Atomic number is ____________________________________________________________________

o Example if I have 12 Protons that would be my atomic number

Hunnicutt Unit 2: Atoms and Elements 8

Isotopes Isotopes are: _________________________________________________________________________ Example:

Mass Number Mass number is _______________________________________________________________________

Mass number is measured in ____________________ _____________________ __________________

Each proton and neutron is ______ amu

o Example: 3 protons and 4 neutrons would have a mass number of 7amu

Atomic Mass• ____________________________________________________________________________________

• The average considers the percent _______________________ of each ___________________ in

nature

• Found on the __________________________ table of elements

• Example:

Hunnicutt Unit 2: Atoms and Elements 9Lesson 2: Periodic Table

Hunnicutt Unit 2: Atoms and Elements 10Mendel

Hunnicutt Unit 2: Atoms and Elements 11• Mendeleev was the ______________________________ scientist to notice the relationship between

the elements

• Arranged his periodic table by ________________________________________

• _________________ 1st Periodic Table

• _______________________ 2nd Edition Published

• ________________________ give elements their _______________________________

Information in the Box

Use of the Periodic Table• Atomic number increases from ____________________________ to __________________________

• Class of elements

________________________ , __________________________, and

_______________________

• Properties can be predicted from the __________________________ of the element

Periods

Groups

Atomic Number = # of protons

• __________________________ : found between the atomic number and atomic mass

• Contains 1 to 2 letters of the __________________ or _________________ names

____________________ = # of protons plus neutrons

Each row is called a “__________________”

The elements in each period have the

________________ number of

________________ levels

1st Period = 1 E. Level 2nd Period = 2 E. Levels3rd Period = 3 E. Levels 4th Period = 4 E. Levels5th Period = 5 E. Levels 6th Period = 6 E. Levels7th Period = 7 E. Levels

Hunnicutt Unit 2: Atoms and Elements 12

Day 1 Review1. Who came up with the periodic table and what did he discover?

2. What is a period and what is a group?

Day 2Valence Electrons• Have _____________________________ energy

• Involved in __________________________________

• Number of valence electron _________________________________ chemical properties

Electron Dot Diagram

• Each _______________________________ has a _________________________ number of valence electrons

• 1-8 valence electrons

Each column is called a

“_________________”

Each element in a group has the

______________ number of electrons

in their outermost

_________________ level (valence

electrons)

Hunnicutt Unit 2: Atoms and Elements 13Bonding• More stable is they have _____________ valence electrons

• Valence electrons can be ________________________ or _________________________

• Chemical bonds

______________________________________________________________________________

______________________________________________________________________________

Noble Gasses• ________________________________________

• ________________________________________

• ________________________________________

Metals• Elements in the _____________________________ section

• React by ____________________________their valence electrons

• _________________________________ from left to right

• Alkali Metals

______________________________________________________________________________

______________________________________________________________________________

Nonmetals• Orange section

• _______________________ or _________________________ electrons

• Combine with ____________________________ by __________________________ electrons

• Halogens

• React ________________________________ with other elements

• 7 valence electrons

Metalloids• Lie along a ______________________ line

• Between __________________ and ___________________

• Has ________________________________ of both

Day 2 Review

Hunnicutt Unit 2: Atoms and Elements 14Metals Nonmetals Metalloids Noble Gasses

Location on Periodic table

Hunnicutt Unit 2: Atoms and Elements 15What do they do with their valence electrons?

How reactive are they?

Give some examples

Draw a dot diagram for the element Oxygen, Argon, Gold.

Hunnicutt Unit 2: Atoms and Elements 16Lesson 3: Matter and MixturesSC Standards• 7.P.2.A Conceptual Understanding: All substances are composed of one or more elements. Elements

are pure substances which contain only one kind of atom. The periodic table organizes these elements based on similar properties. Compounds are substances composed of two or more elements. Chemical formulas can be used to describe compounds.

• 7.P.2A.3: Analyze and interpret data to describe and classify matter as pure substances (elements or compounds) or mixtures (heterogeneous or homogeneous) based on composition.

• 7.P.1A.4: Analyze and interpret data from informational texts, observations, measurements, or investigations using a range of methods (such as tabulation, graphing, or statistical analysis) to (1) reveal patterns and construct meaning or (2) support hypotheses, explanations, claims, or designs

Lesson 3 Objective (SWBAT)• analyze and interpret data to describe and classify matter as pure substances or mixtures based on

composition.

Day 1: Matter

What is Matter• ____________________ BC Empedocles

• Proposed that all matter was made of 4 elements, _________________________________________________

• _______________ ’s • Discovered that it was ___________________ than 4 elements

Elements• All matter made from more than ______________________ different substances

• ____________________________________________________________________________________

____________________________________________________________________________________

• ___________________________ substance

• Identified by __________________________ and ___________________________ properties

Atoms• ____________________________________________________________________________________

____________________________________________________________________________________

• _____________________________ charged nucleus

• Surrounded by a ____________________ charged

electron _________________________

• Made of

• ____________________________________________

• ____________________________________________

Hunnicutt Unit 2: Atoms and Elements 17• ____________________________________________

• The number of ________________________________ give the atom its

___________________________

Molecules• Chemical Bonds

• ______________________________________________________________________________

• ______________________________________________________________________________

• ______________________________________________________________________________

• A molecule is _______________________ or ___________________ atoms

held together by chemical bonds

• Example:

• H20, CO2, O2, C6H12O6

Compounds• Compound

• ______________________________________________________________________________

______________________________________________________________________________

• When elements ___________________________ they can have very ________________________

properties then the ____________________________________ elements.

Chemical Formula• Chemical Formula

• ______________________________________________________________________________

______________________________________________________________________________

• How many Carbon, Oxygen, and Hydrogen atoms are in C6H12O6?

Day 1 Review

1) What is matter? (Think back to Unit 1)

2) What are the three parts of an atom and what are their charges?

Hunnicutt Unit 2: Atoms and Elements 183) What would be the chemical formula if you had a mixture:

a. One sodium and on chlorine

b. One chromium and two potassium

c. Two hydrogens and one oxygen

Day 2: Types of Mixtures

Mixtures• Made from _________________________ or ___________________________________ substances

• Found ________________________________ at the same ____________________________ and

same _____________________________

• Each substance __________________________________ its own properties

• Two types

• ______________________________ and _____________________________ Mixtures

Heterogeneous• ___________________________ see the ____________________________________ parts

• Can ____________________________________ be separated

• Examples

• ______________________________________________________________________________

______________________________________________________________________________

Homogenous Mixtures• Are _________________________________ mixed

• _________________________________________ be easily separated

• Examples:

• ______________________________________________________________________________

______________________________________________________________________________

Day 2 Review1) What is a mixture?

Hunnicutt Unit 2: Atoms and Elements 192) What are the two types of mixtures?

3) Describe and give examples of each type of mixture.

Lesson 4: Ionic and Covalent Bonds

SC State Standards

• Standard 7.P.2: The student will demonstrate an understanding of the structure and properties of matter and that matter is conserved as it undergoes changes.

• 7.P.2.A Conceptual Understanding: All substances are composed of one or more elements. Elements are pure substances which contain only one kind of atom. The periodic table organizes these elements based on similar properties. Compounds are substances composed of two or more elements. Chemical formulas can be used to describe compounds.

• 7.P.2A.4: Construct explanations for how compounds are classified as ionic (metal bonded to nonmetal) or covalent (nonmetals bonded together) using chemical formulas.

• S.1A.6: Construct explanations of phenomena using (1) primary or secondary scientific evidence and models, (2) conclusions from scientific investigations, (3) predictions based on observations and measurements, or (4) data communicated in graphs, tables, or diagrams.

At the end of the lesson Students will be able to…

• Construct explanations of how compounds are classified as ionic or covalent using chemical formulas.

Day 1 Ions and Ionic Bonds

What is an Ion?

• Ion

• ______________________________________________________________________________

______________________________________________________________________________

• Happens

• When a neutral atom _________________________________ a valance electron

• The atom will become _______________________

• When a neutral atom ______________________________ a valance electron

• The atom will be ___________________________

• _________________________ tend to ______________________

• ___________________________ tend to _______________________________

Hunnicutt Unit 2: Atoms and Elements 20Common Ion

• Some ions are made of __________________________________ atoms

• Polyatomic ions

• ______________________________________________________________________________

______________________________________________________________________________

• Are ____________________ or ____________________

Ionic Bonds

• Happens when atoms easily ____________________________ and electron and other

____________________ an electron

• ____________________ ___________________________ are transferred from one atom to another

• Example:

• Na will _______________________ an electron and become _____________________

• Cl will __________________________ an electron and become ________________________

• Ionic Compounds

• Made up of ______________________ and ___________________________ ions

• Positive ions will _________________________________ negative ions

Hunnicutt Unit 2: Atoms and Elements 21Ionic Chemical Formulas

• Chemical Formula

• ______________________________________________________________________________

______________________________________________________________________________

• If ________________________ subscript ______________________________ the number is

________________________

Brain Break

1. What is an ion?

2. What are ionic bonds?

3. What is a chemical formula?

Naming Ionic Bonds

• Name of the ____________________________________ ion comes ______________________________

• The name of the ____________________________________ ion come ________________________

Properties of Ionic Compounds

• Form _________________________ brittle crystals that have _______________________ melting points

• Conduct _______________________________ when ______________________________ in water or melted

• Ionic crystals

• Form solids by ______________________________up ________________________ patterns of ions

• Crystals: ________________________________________________________________

_______________________________________________________________________

• Ions are _______________________________ to ion of an opposite

_______________________________

• High Melting Point

Hunnicutt Unit 2: Atoms and Elements 22• Take a lot of _______________________________ to break apart ion

____________________________

• Melting point of NaCl is ________________________

Day 1 Review Questions

1. An atom that loses a valance electron become a (positive/negative) ion. An atom that gains a valance electron becomes a (positive/negative) ion

2. Determine the number of atoms of each element in the chemical formula Na2S

3. Ionic bonds are strong enough to cause almost all compounds to be

_____________________________ at room temperature.

Day 2: Covalent Bonds

Covalent Bonds

• Covalent Bonds

• ______________________________________________________________________________

• ______________________________________________________________________________

• Electron Sharing

• ______________________________________________________________________________

______________________________________________________________________________

• ___________________________ in nucleus of each atom ________________________ the atoms together

• Molecule

• ______________________________________________________________________________

______________________________________________________________________________

Hunnicutt Unit 2: Atoms and Elements 23

How Many Bonds?

1. ____________________________________________________________________________________

____________________________________________________________________________________

2. ____________________________________________________________________________________

____________________________________________________________________________________

• Examples

• H=________________ valence electron=________________________ bond

• C=________________ valence electrons=_____________ bonds

• O=________________ valence electrons=_____________ bonds

• Double Bonds

• ______________________ atoms share ___________________ pairs of electrons

• Triple Bonds

• __________________ atoms share ____________________ pairs of electrons

Hunnicutt Unit 2: Atoms and Elements 24Brain Break

1. What is a covalent bond?

2. How is it different then an ionic bond?

3. How many bonds can you have in a covalent bond?

Properties of Molecular Compounds

• Molecular Compound

• ______________________________________________________________________________

______________________________________________________________________________

• ______________________________________________________________________________

______________________________________________________________________________

• Do _____________________________ conduct electricity when melted or dissolved in water.

• Have __________________________ melting and boiling points

• Do ___________________ contain ______________________ particles

• ______________________________ bonds then ionic

• Table sugar melts at 190C table salt melts at 801C

Partially Charges

• Atoms of some elements have ______________________ pull then others

• ___________________________ sharing of electrons

_______________________ covalently bonded atoms to have

__________________ electric charges

Nonpolar and Polar Bonds Nonpolar

o Each _____________________ pulls on the ___________________________ the

________________________

Hunnicutt Unit 2: Atoms and Elements 25o Electron are ________________________ equally

Polar Bonds

o When ____________________________ atom has a ________________________ stronger pull

on the _____________________________________

o The ______________________________ atom will be ___________________________

negative

o The _______________________________ atom will be slightly positive

Van der Waals Forces Van der Waals Forces

o ______________________________________________________________________________

______________________________________________________________________________

_____________________ melting and boiling point

Example

o Water

Day 2 Review1. Draw an electron dot diagram for 1 iodine atoms

2. Water is an example of a(n) (ionic/molecular) compound.

3. When do molecular compounds form?

4. Sodium chloride is an example of a(n) (ionic/molecular) compound.

5. Ionic compounds form when…