Biology Summer Work 2015: This packet has been put together by your

Biology teachers for you to work on during the summer. It will help you

review topics that you have learned in 9th grade and will help you be

successful in Biology.

This packet will be due on Thursday, September 3, 2015. Please expect

to take the test on Wednesday, September 9, 2015.

Name: __________________________________

9th Grade Teacher: _______________________________

Chemistry Review Name _____________________________

Lesson 1: Atomic Structure

Basic Atomic Structure http://www.youtube.com/watch?v=lP57gEWcisY

What are Atoms? (text w/music) http://www.youtube.com/watch?v=jZO6W-DEVLk&feature=fvwrel

Atomic Symbols http://www.youtube.com/watch?v=7JiiSPxiuAc&feature=related

Notes: (Your Biology teacher expects to see notes for every clip)

1. Identify the three types of particles that make up an atom and their charges:

Particle Charge of particle

2. The Nucleus – contains ____________________________ and ____________________________

3. The space that surrounds the nucleus and contains electrons is called the _____________ _____________

4. What keeps electrons from just shooting off away from the atom? (video #1).

5. A neutral atom has the same number of ____________________ and __________________________.

6. The word atom means ______________________.

7. When comparing the mass of these particles, _________________ and __________________ have a mass of 1

atomic mass unit (AMU) while the mass of ______________ is 1/2000 AMU. Therefore, when calculating the

mass of an atom, only the mass of the _______________ and _________________ are considered.

ATOMIC NUMBER Elements are identified by the number of p+ they contain.

8. If an atom has 11 p+, it must be _____________.

9. If an atom has _____ p+, it must be N.

10. H has _______ protons, _____neutrons and _______electrons.

11. Complete the table below using a periodic table (online or in your agenda pad)

Element Name

Element Symbol

Atomic # # Protons # Neutrons # Electrons Mass #

Lithium Li 3 6

C 6 6 12

23 23 23

12. Atoms that exist and combine with other dissimilar atoms are called __________________.

13. Elements are made up of _______________ and compounds are made of of molecules.

Atomic #

Symbol

Name

Atomic Mass

30

__________

Zinc

65.39

3

Li

___________

6.941

Chemistry Review

Lesson 2: Atoms, Isotopes and Ions Atoms and Isotopes: http://www.youtube.com/watch?v=SeDaOigLBTU

What are Isotopes? http://www.youtube.com/watch?v=EboWeWmh5Pg

Protons/neutrons/electrons in atoms/ions from mass/atomic number and charge http://www.youtube.com/watch?v=SoMNy2fAoiE

Notes: (Your Biology teacher expects to see notes for every clip)

1. An isotope is a different _______________ of the same _______________.

2. Isotopes and atoms of an element have the same # of ____ but different numbers of _____.

3. Ions are atoms with unequal number of ______ and _______.

Neutral Atoms:

1. The # of __________________ and # of ____________________ are equal.

2. A neutral oxygen atom has 8p+. How many e- will it have? ________

3. How many p+ and e- does a neutral Calcium atom have? _________

Stability # of protons never changes for a given element; only e- are lost or gained.

4. When the # of p+ no longer equals # of e-, the atom is an: ________________

5. An excess # of e- means the atom has a ____________________charge

6. Fewer e- than p+ means the atom has a ____________________ charge

7. Complete the table below using a periodic table (online or in your agenda pad)

Element Name

Element Symbol

Atomic # # Protons # Neutrons # Electrons Mass # Charge +/-/o

Iron 26 52

8 8 9

23 23 23

Hg 80 80 200

8. If you know only the following information can you always determine what the element is? (Yes/No).

a) number of protons ___________

b) number of neutrons___________

c) number of electrons in a neutral atom___________

9. The number of protons in one atom of an element determines the atom’s _____________ ______________, and

the number of electrons determines the ___________________of an element.

10. The atomic number tells you the number of _____________________in one atom of an element. It also tells you

the number of _____________________in a neutral atom of that element.

11. The atomic number gives the “identity “of an element as well as its location on the Periodic Table. No two

different elements will have the same _____________ ______________.

12. The ______________ _______________of an element is the total number of protons and neutrons

in the___________________ of the atom.

13. The ______________________of an element is the average mass of an element’s naturally occurring atom, or

isotopes, taking into account the ______________________of each isotope.

14. The mass number is used to calculate the number of ___________ and ___________in one atom of an

element. In order to calculate the number of neutrons you must subtract the ___________from the

_________________.

15. Complete the table below.

Ion Symbol Element

Name # Protons # Electrons Charge Anion/Cation

H1+

S 2-

K 1+

Chemistry Review

Lesson #3: Period Table and Lewis Dot Diagrams

A Tour of the Periodic Table http://www.youtube.com/watch?v=fLSfgNxoVGk&feature=related

Notes: (There is a lot in this video; groups periods, gallium, reactivity, halogens etc.) Periodic Table Part II: How to use the table http://www.youtube.com/watch?v=wGz7uqMxddQ&feature=related

Notes: at least three points not mentioned above

Drawing Lewis Dot Diagrams http://www.youtube.com/watch?v=ulyopnxjAZ8 Notes: be specific – this will help with the table on page 3

Answer the following questions: 1. In the periodic table, the vertical columns are called ___________________, while the rows are called

_____________________.

2. Color the following groups on the periodic table below with the corresponding colors

Alkali Metals - yellow Halogens - orange

Alkaline Earth Metals – green Noble Gases - red

3. The number of electrons in the outer energy shell of a particular atom are called _________________ electrons.

4. What are two ways to determine the number of valence electrons a particular atom has? Hint: One is much easier

than the other.

a)

b)

5. The Alkali metals are ( circle one) Highly/ Non reactive, and all have _____ valence electron(s)

6. The Alkaline Earth metals have _____ valence electron(s).

7. The Halogens have ____ valence electrons, thus they are (circle one) Highly/ Non -reactive.

8. The Noble gases have _____ valence electrons, making them (circle one) Highly/ Non -reactive.

9. Circle the non-metals on the periodic table above.

10. Why are these non-metals, known as “CHNOPS”, so important to Biology? Here’s the big connection!!!

11. Label the transition metals using a large bracket on the periodic table above.

12. Draw a zigzag line along the metalloids…you should remember this from last year!

13. As we move towards the bottom of the periodic table, the atomic mass. (increases/decreases).

14. As we move across a row, the atomic mass. (increases/decreases) because ____________________

Bohr Diagrams:

The Bohr Diagram is used to show the exact number of electrons for a particular atom of an element. The images below show Bohr Diagrams of Carbon.

You Try: In the space provided, draw the Bohr diagram for Chlorine (Cl).

a) How many valence electrons does an atom of Chlorine have?

b) How did you know this by looking at your Bohr diagram?

Electron Configuration and Stability

Every atom wants to be stable, and stability for an atom is achieved by having the right number of electrons in its outermost shell. Atoms that already have the ideal number of electrons in their outer shell have no desire for more electrons, and don't want to lose any either. These atoms tend to be un-reactive or inert.

Atoms that that do not have the ideal number tend to be reactive, striving to get their hands on more, or get rid of some electrons. The atom will strive to achieve stability by gaining or losing electrons in their outer shell. If this cannot be achieved by shuffling their own electrons around, atoms interact or react with other atoms to take/ give (ionic bonds) or share (covalent bonds) electrons to achieve their goal. Atoms that that do not have the ideal number tend to be reactive, striving to get their hands on more, or get rid of some electrons.

The table below lists shells one to five, and shows the maximum number of electrons each shell can hold. Remember, a

full shell makes a happy atom. We will only be working with 3 shells this year!

Shell Can hold is stable with an outer

shell holding

1 2 2

2 8 8

3 18 8

4 32 8

5 50 8

Lewis Dot Diagrams: It’s really tedious and downright “Bohr-ing” (get it?) to draw out all of those rings, so we usually

show valence electrons using the Lewis Dot Diagram. Watch the tutorial on drawing Lewis Dots and complete the table

below.

Element

Name Symbol Protons Electrons

How many

shells?

E-

in the outer shell Lewis Dot Model

show electrons in outermost shell

Hydrogen H 1 1 1 1 H

Helium He 2

Lithium Li 3 2 1

Beryllium Be 4 4

Carbon C 6 6

Oxygen O 8 8 2

6

Fluorine F 9

Neon Ne 10 10

Sodium Na 11 11

Magnesium Mg 12 12

Chlorine Cl 17 3

7

Argon Ar 18 18 3 8

Chemistry Review

Lesson #4: Bonding

Bond's in Biological Molecules -

http://www.kentchemistry.com/links/bonding/bondingflashes/bond_types.swf

Notes: (Your Biology teacher expects to see at least three concepts)

Intro to Chemistry: Intro to Bonding http://www.youtube.com/watch?v=NT_42EQmQRo&feature=related

1. What do Bonds do? ________________________________________________________________

2. Ionic Bonds produce _____________.

3. Draw the Lewis dot structure of Sodium using pen and Draw a Lewis dot structure of Chlorine in pencil.

4. Use arrows to indicate what happens to the electrons when they interact and any charges that result.

5. What types of elements form ionic bonds? __________________________________________

6. Another term of covalent bond is _________________________________

7. In covalent bonding, electrons are ________________________________

8. Draw the Lewis dot of two hydrogen atoms, one in pen and one in pencil. Circle the shared electrons.

9. Redraw this molecule using a line to represent the covalent bond.

10. What type of molecules form Covalent bonds? ________________________________________

Intro to Chemistry: Ionic Bonding 2: http://www.youtube.com/watch?v=SqI3glG98O0&feature=relmfu

11. When atoms bond ionically, one atom ________ electrons and another atom __________ electrons.

12. If the first atom gives away 2 electrons, the charge of the atom will be __________. The charge of the

atom that received the electrons will be__________.

13. How to these charged atoms behave toward one another and why?

__________________________________________________________________________________________

______________________________________________________________________________

14. What does the word "salt" mean to a chemist?

____________________________________________________________________________________

____________________________________________________________________________________

15. List some characteristics of Ionic Compounds

____________________________________________________________________________________

____________________________________________________________________________________

Intro to Chemistry: Covalent Bonds ½ http://www.youtube.com/watch?v=6_YhSLnAmVo

16. What attracts two molecules toward each other in covalent bonds?

____________________________________________________________________________________

____________________________________________________________________________________

Notes: (numerous definitions – including polar and non-polar covalent bonds)

Ionic and Molecular Compounds http://www.youtube.com/watch?v=LRVW0tgSLRI

Notes:

That's Why Carbon Is a Tramp: Biology #1

http://www.youtube.com/watch?v=QnQe0xW_JY4&feature=relmfu

17. What are organic molecules?

18. The atomic # of C=______.

19. How does being small benefit carbon?

20. What does it mean when we say "carbon is kind"?

21. What does the speaker mean when saying "Carbon is a tramp"?

22. What is the octet rule?

23. Carbon it requires ______ electrons to fill its outer orbital.

24. Draw a Lewis dot diagram of 1 carbon using a pen. Surround it with 4 Lewis dot diagrams of hydrogen

using pencil.

25. Show how electrons are shared between these atoms.

26. What is the chemical formula for the molecule you just drew?

27. What is the difference between non-polar and polar covalent bonds?

28. Why do oxygen molecules "stick together"?

29. In general, which type of bond is the strongest? __________________________________

Episode 1: Global Warming, It's All About Carbon http://www.youtube.com/watch?v=ypbb9Zi5Tao&feature=relmfu Notes:

Episode 2: Global Warming, It's All About Carbon

http://www.youtube.com/watch?v=cOJ3MUpDrfI&feature=relmfu

Notes:

30. Create a Lewis Dot diagram for the compound KCl. Is this ionic or covalent? ______________ Label any

charges

31. Create a Lewis Dot diagram for MgCl2. Is this ionic or covalent? ______________ Label any charges

32. Create a Lewis Dot diagram for NH3. Is this ionic or covalent? ______________ Circle any shared electrons

33. Create a Lewis Dot diagram for CH4.Is this ionic or covalent? ______________ Circle any shared electrons

34. Create a Lewis Dot diagram for H20. Is this ionic or covalent? ______________ Is this polar or non-polar?

___________