Chemistry of Life (Chapter 6 Pages 144-170)

Name:________________________

Hr.:_______

Section 1: The Atom

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• ____________ = smallest piece of ________________ that still regains the property of the _________________

True or False: All matter is made up of atoms

For example:

• Hydrogen is composed only of ________________atoms, silver is only composed of ______________atoms, etc

• Atoms are composed 3 of ____________________ particles:

– __________________________

– __________________________

– __________________________

Sub-atomic Particle

Definition Location Charge

Proton

Neutron

Electron

Are protons, neutrons, and electrons the smallest particles that can exist?

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• _____________________ are not composed of smaller particles (one of the most basic types of particles)

• ___________________ and _________________ are made up of smaller particles called _______________

Section 2: Mass of an Atom

• ___________________ _________________

– Most of the _________________ in an atom is contained in the ___________________

• _____________________ and __________________ are far more massive than electrons

• Mass of an ____________________ is so small, that it is not taken into account when measuring ________________________

Atomic mass unit (______________ )- _______________________________________________________________ ________________________________________________________________________________________________

• Equals about the mass of a ________________________ or ____________________

Wildcats Share

• Answer the following questions, by referencing to the front page of your note packet.

1. Does every element within the table have the same AMU?

2. Does every element listed have the same atomic number?

3. Why do you think these are all the same or different?

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• Every _______________ is different because they have a different number of ________________

– Number of ___________________ tells you what type of element you have

– Atomic number of carbon= _________, therefore carbon has _________ protons

• __________________________ = the sum of the number of ___________________ and ______________in the nucleus of an atom

• Example

– Mass number of carbon=_________, therefore there must be ______ neutrons and ______ protons

Wildcats Share

• Solve the following within your groups.

1. If Boron has a mass number of 10, with 5 protons, then how many neutrons does it contain?

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2. The atomic number of Chlorine is 17, therefore how many protons does it contain?

3. Magnesium has a mass number of 24, with 12 neutrons, what would the atomic number of magnesium be?

How do you name an element?

• Naming Elements:– _________________________________ for elements can stand for several different

things• First letter(s) of the ____________________ ____________________• First letter(s) of the ________________________ name for the element

– Example: _____________________________________________________________

• Some elements named for ____________________________• Other named for _____________________ or_____________________

– All these ___________________ are used world-wide, so everyone understands what the symbols mean

_________________________

• Atoms of the ___________________ element that have different numbers of _____________________

• Examples:

– Carbon-________= most common form of carbon

– Carbon-________= carbon atoms with ______extra neutrons

• ___________________________5

• Because they have the same number of __________________, all isotopes of an ___________________ have the same chemical properties.

• __________________________________ = weighted average mass of the mixture of its ___________________

• Example: Boron- ______ and Boron-_______

– ______ out of ______ boron atoms are Boron- 11

– To find the average atomic mass:

Section 3: The Periodic Table

• In the late 1800’s,________________________, a Russian chemist, searched for a way to organize the __________________

– He Organized elements in order of ______________________ atomic number

– Noticed a _____________________

– ________________________: elements are arranged by increasing atomic number and by changes in _________________and ____________________ properties

• _______________________________________

• What is the electron cloud?

• In a _________________ atom (no charge) the number of neutrons __________________ the number of ___________________

• Electrons in the cloud have different amounts of _______________ depending on which _____________ they occupy

– Closer to the ________________ the electron, the _______________the energy of the electron

– Electrons fill the energy levels starting at the ______________ levels (near the nucleus) then fill the ___________________ levels

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• Elements with the same number of _________________ in their outer layer are in the same ________________ and have similar ______________________

• __________________ elements will contain _________ electrons in their __________________________shell

– Outer most electrons=________________________________

Wildcats Share

Use the color pencils at your desk to color the sulfur atom below.

• Nucleus = blue

• Electrons= green

• Circle the electrons that are found within the valence shell.

What is the atomic mass of sulfur?

What is the number of protons and neutrons?

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Organizing the Periodic Table

• ________________ (families)= _____________________columns in the periodic table

– Numbered __________________

– Elements in each group have ____________________ properties

– Example: group _______(copper, silver, and gold) are all shiny and good conductors of electricity and heat

• What is responsible for these similar properties?

__________________________________________________________________

• ________________ on the Table

– Notice: row one only has ___________________ and ____________________

• Hydrogen= _______ electron, helium= _______electrons

– Since the first shell can only hold ________ electrons, helium has a __________ outer shell and is happy

• Row _______ starts over with__________________, which has _________ electrons…

– End of each row is an __________________ that has ________ valence electrons

Wildcats Share• Turn to the front page of your note packet.• From here we will color code your periodic table of elements for how many electrons will be

held within the valence shell.– At the top of your page provide the following key-

• Green= 1 electron

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• brown= 2 electrons• Blue= 3 electrons• Red= 4 electrons• Purple= 5 electrons• Yellow= 6 electrons• Black= 7 electrons• Orange= 8 electrons

_________________ Group, ____________________ Properties

• Example: group 17, the _________________________

– All have ______ outer electrons

– All will undergo _____________________reactions in the same way

– All have the ability to form _________________ with elements readily with elements in group _______ _______

• ____________ : a substance formed by the chemical combination of 2 or more elements

– Elements in group _______________ all have _____ valence electron

– For Example:

• Na (______________) and Cl (_____________) bond easily to form table salt (______________)

• Group _________ have _____ valence electrons which make them unreactive

• __________________on the Periodic Table

• ___________________ = horizontal rows of elements on the periodic table that increase by one _____________ and one _______________ as you go from _______________to ________________

– ________________________________________________________________________

Section 4: Bonding

• _______________ ________________: tells what elements a compound contains and the exact number of the atoms of each element in the compound

• Example-

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– What is the chemical symbols and chemical formulas for the following?

• What does the H2 mean? – The “little” 2 is a ____________________

• A subscript written after the __________________, tells you how many ____________ of that element are in a unit of the compound

• If a symbol has no _______________, then the unit only contains ______ atom of that element

• So how many atoms of each element were involved within the compound of NaCl?

• So how many atoms of each element were involved within the compound of H2O?

• __________________ ___________________– Occurs when the __________________ ____________ level has a maximum number of

_____________– Outer energy levels of _______________ and _________________ are stable with

______ electrons– All other ____________________ are stable or “happy” with _______ electrons

• So why are Nobel gases always “happy” or considered unique? __________________________________________________________________

• _________________ ______________- getting their fill– So how does Hydrogen or any other element without a full outer energy level become

stable? – _______________ with partially stable outer energy levels can

• _____________ electrons10

→ +

Sodium Chloride → + Chloride Sodium

→ +

Water→ + Oxyge2Hydrogen

• _____________electrons• _____________electrons

– they do this by ____________________ within other atoms with partially complete _______________ _______________ __________________

– As a result of this combination they become __________________• Which makes them

• _______________ - lose or gain ________________ to become _________________– An atom that has _____________ or ___________ an electron is called an __________

• ____________ - is a _______________ particle because of having lost or gained an electron, which causes it to have _____________ or ______________ electrons than protons

• This means: __________________________________________________________

• These _______________ _______________ between oppositely charged particles, such as _________, that hold _____________________ together

• Ionic bond= _____________________________________________________________________________ _________________________________________________________________________________________

– _________________ of 1 or more ___________________ takes place – Large amount of _____________________________________________________

• Usually formed by combining ______________________________________________________________

• Example: group _______________________________ • Ionic compounds=

_________________________________________________________________________ _________________________________________________________________________

• Covalent bond= ___________________________________________________________________________ _________________________________________________________________________________________

– Covalent compounds= _________________________________________________________________

• Molecule= _____________________________________________________________________________

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____________________________________________________________________________________________

Section 5: Chemical Reactions

________________________________• always involve the ________________ of ____________ in reactants and the

formation of new ___________ in the products• ____________________= are the _____________ or _________________ that

enter into a chemical reaction• ____________________= are the ______________ or ________________ that

are formed after the chemical reaction has occurred

CO2 + H2O → H2CO3

• Chemical reactions that _____________ ___ often occur all of the time • however, chemical reactions that __________________ will not happen unless a

source of _____________ is available • Not all chemical reactions happen automatically, most often they require

____________• the energy that is needed to get a reaction started is referred to as the

____________________ ___________

______________• a substance that ______________ up the rate of a reaction

__________________• are ______________ that act as biological _____________• cells use enzymes to _____________ up chemical reactions that take place within the

cell • this occurs by ________________ the activation energy that is needed

Chemical Properties

• _________-a combination of substances in which the individual ___________ retain their own __________.

– Example: 12

• _________- a mixture in which one or more substances (________) are distributed ________ in

another substance (________) – Example:

• The more solute that is dissolved in a given amount of solvent, the ________ the solution’s ____________ (strength)

• Organisms can’t live unless the _________ of dissolved substances stays within a _________, _______ ______

• Organisms have many __________ to keep the concentration of __________ and ions within this range

• Chemical reactions in organisms can depend on the ____ of the ___________.• ____- a _________ of how _______ or ______ a solutions is.

• A scale with values ranging from ___ to ___ is used to measure pH.• ______- substance with a pH _______ 7 and that forms _________ ions in water • ______- substances with a pH _______ 7 and that forms _________ ions (OH-)

Elements Important do Life• Water is necessary for many of life’s _________ and _______ ________• Water is a ______ ______

• These molecules occur when there is an ________ sharing of electrons which results is each molecule having a ________ end and a ________ end

• Water molecules attract each other, as well as _____ and other ______ ________, because of this water can dissolve many ______ ________ and many other _________ _______

• _________ _____-weak. Chemical bond formed by the attraction of __________ charged hydrogen atoms to other _________ charged atoms

• Because of its ________ water has the unique property of being able to ______ up thin tubes. This property is important within ______

• Water resists ________ in ____________• This property helps cells _________ an optimum environment • _________- the net __________ of particles from an area of _______ concentration to an area

of _______ concentration • Diffusion is a ______ process because it relies on the _________ molecular motion of ______• Three key factors ____________, ____________, and _________ affect the rate of diffusion• The more ___________ the substances, the more rapidly ________ occurs• Increasing ___________ and ________ increase particle motion and increase diffusion • _________ _________-result of diffusion where there is __________ movement of particles

but no overall change in ___________ • The difference in _____________ of a substance across space is called a __________

_________• Because ions and molecules diffuse from an area of _______ concentration to an area of

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______ concentration they are said to move ______ the gradient• Diffusion is one of the ________ by which cells move __________ in and out of the cell • Draw a diagram to show diffusion and dynamic equilibrium

Name:______________________________

Hr.:_____________

Unit 2: Chemistry of Life Vocab

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Instructions: Define the following terms below.

Term Definition

1. Chemical Reaction

2. Atom

3. Periodic Table

4. Average atomic mass

5. Proton

6. Electron

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7. Period

8. Nucleus

9. Mass number

10. Isotope

11.Neutron

16. Catalyst

17. Enzyme

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18. Activation Energy

19. Ionic Bond

20. Covalent Bond

21. Compound

*This would be a great sheet to review before the Vocab Quiz!

Name:____________________

Hr.:_____

Section 1: Homework

1. Chemical symbols can stand for: a. The first letters of the element nameb. The first letters of the Latin name for the elementc. A person d. A place or propertye. All of the above

2. All matter is made of:

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a. Moleculesb. Organic elementsc. Hydrogend. Atoms

3. Write out the definition of an atom: ___________________________________________________________ ________________________________________________________________________________________

4. Neutrons have a ________ charge. a. Positiveb. Negativec. Neutral

5. Electrons have a _______ charge. a. Positiveb. Negativec. Neutral

6. Protons have a _______ charge. a. Positiveb. Negativec. Neutral

Fill in the following table:

Subatomic particle Location Charge

Proton 7. 8.

9. 10. Negative

11. Nucleus 12.

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Name: ______________________

Hr.:______

Periodic Table

Use your periodic table and circle the word(s) that best complete the following sentences:

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1. Calcium and potassium are in the same (period) (group) on the periodic table. 2. Nitrogen and carbon are in the same (period) (group) on the periodic table. 3. Fluorine and bromine are in the same (period) (group) on the periodic table. 4. Copper and silver are in the same (period) (group) on the periodic table.

________________________________________________________________________________________________

Fill in the blank with the correct number:

5. Lithium has ______ valence (outer) electrons. 6. Xenon has ______ valence (outer) electrons. 7. Magnesium has ______ valence (outer) electrons. 8. Sulfur has ______ valence (outer) electrons. 9. Tin has ______ valence (outer) electrons.

________________________________________________________________________________________________

Complete the electron dot diagram for the following elements:

Sr K Ga Kr Br Se

Sb Si C H He Fr

Mg I As Rn Cl Te

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