Name: __________________________________ Period:_________ Date: ________________
Atom Review Worksheet
Complete the following chart:
Particle
Location
Nucleus
Mass
Large
Charge
positive
Nucleus
Large
No charge
Outer shell
Small- does not
contribute to mass #
negative
Proton
Neutron
Electron
Find the Missing Numbers (you should know how to find the information to complete the table below)
Element
Atomic
Number
Mass
Number
# of
Protons
# of
Neutrons
# of
Electrons
Iron
26
56
26
30
26
Sulfur
16
32
16
16
16
# of
Valence
Electrons
[Ar]4s23d6
Chemistry
next year!

6
Carbon
6
12
6
6
6
4
Fluorine
9
19
9
10
9
7
Calcium
20
40
20
20
20
2
Nitrogen
7
14
7
7
7
5
Copper
29
64
29
35
29
Chemistry
next year!

Remove Iron and Copper- you will learn the transition metals next year in chemistry!

What is a covalent bond?
A bond formed by the sharing of electrons between two atoms (example: CH4)
What is an ionic bond?
A bond formed between two charged atoms (ions) (example: Na+ + Cl-
NaCl)
Isotope or Different Element?
In each of the following statements, you are given a pair of elements and important information about
each. Use this information to determine if the pair if elements are isotopes or different elements.
Indicate your answer in the space below (either write Isotope or Different Element).
1. Element D has 6 protons and 7 neutrons.
Element F has 7 protons and 7 neutrons.
____element__________________
2. Element J has 27 protons and 32 neutrons.
Element L has 27 protons and 33 neutrons.
____isotope_________________
3. Element X has 17 protons and 18 neutrons.
Element Y has 18 protons and 17 neutrons.
____elements__________________
4. Element Q has 56 protons and 81 neutrons.
Element R has 56 protons and 82 neutrons.
____isotope________________
5. Element T has an atomic number of 20 and
an atomic mass of 40.
Element Z has an atomic number of 20 and
an atom mass of 41.
____isotope__________________
6. Element W has 8 protons and 8 neutrons.
Element V has 7 protons and 8 neutrons.
____elements__________________
7. Element P has an atomic number of 92 and
an atomic mass of 238.
Element S has 92 protons and 143 neutrons
____isotopes_________________
Name: ______________________________________ Period:_____ Date: _______________
Ions Review
1. What is an ion?
Atoms typically have NO CHARGE since electrons (negative) = protons (positive). When an
atom either gains or loses an electron it will become an ion or a charged atom- (ion: an atom
that either lost or gained electrons/ an atom with a charge)
2. If Oxygen gains 2 electrons from another atom, why is written O-2 (with a -2)?
Since atoms that gain electrons now have two more negatively charged particles compared to
the number of protons (positive charge) that atoms has a -2 charge.
3. If Sodium loses an electron to another atom, why is it written Na +1 (with a +1)?
Since the sodium atom has lost a negative charged particle (electron) it now has one more positive
charged particle (proton) compared to the negative (electron) giving it a +1 charge.
4. Describe the charge on Mg+2 ion. Is it a cation or anion?
Mg has lost two electrons giving it a +2 charge. A positive charged ion is called a CATION.
______________________________________________________________________________
Properties of Water Review
1. Use the following terms to label the molecule below: Hydrogen(H), Oxygen(O), -, +
What type of molecule is it: _____water/polar____________
Oxygen δHydrogen δ+
2. Use the terms polarity, adhesion, and cohesion to explain what causes the water to rise on the
side of a tube.
Due to the polarity of water (which causes a partially positive and partially negative
end) water has the ability to have an attractive force to the sides of a tube, this is adhesion. Since
water is also cohesive (the attractive force between water molecules) it will pull other water along as if
in a long chain.
Use the diagram below to answer questions 3 and 4
3. Describe what is the picture at the right showing?
____hydrogen bonds between water molecules___
4. What type of bond is shown?
Hydrogen bonds: weak bonds that form between the partially positive
(Hydrogen atoms) and the partially negative (oxygen atoms) of a water molecule.
5. Given the concentrations of [H+] and [OH-], how can we determine whether the solution is
acidic or basic?
More [H+] means it is an acid and more [OH-] is a base (or basic)
6. A student mixes strawberry koolaid and water. A pH meter is used to measure pH of 5.4.
What kind of solution is strawberry Koolaid? ACID
7. In the koolaid mixture, what must there be more of, hydrogen ions or hydroxide ions?
Hydrogen /H+
8. A student adds an alka-seltzer to the koolaid and stirs. The pH meter now reads 8.3. What was
released by the alka-seltzer tablet to cause this change?
Hydroxide ions /[OH-]
9. Baking soda is a weak base. Hydrochloric acid is a strong acid. What would happen if these two
were mixed?
The acid would become a weaker acid with a higher pH than before
10. How much more acidic is a substance with a pH of 3 than a substance with a pH of 5. Explain
your answer.
100 because the pH increases by a power of 10, therefore 10 x 10= 100X greater
Organic Chemistry is the study of all compounds that contain bonds between carbon atoms. Carbon
has 4 valence electrons so its bonds are strong. Carbon even has the ability to bond with other carbon
atoms, forming long chains or even rings. Living things are made up of molecules that consist of
carbons covalently bonded to other elements, such as macromolecules.
Macromolecule
(polymer)
Monomer
“building
blocks”
Polymers
Examples
Function
Polysaccharide:
starch & cellulose
Carbohydrate
Proteins
Lipids
Monosaccharide or
simple sugars
Polysaccharides
Disaccharides
Disaccharides:
Sucrose & lactose
Amino acids
polypeptide
Enzymes (lactase)
Glycerol head &
fatty acid tails
Fats
Sterols
Phospholipids
Triglyceride
Cholestrols
Energy
Structural
Transport
Contractile
Protective
Regulatory
Insulation
Energy
Regulation & growth
Cell Membrane component
Directions: In the space provided, identify the following molecules:
Phosphate
1. ________Monosaccharide______________
3. ______Fat/Triglyceride___________
2. ___________Phospholipid___________
4.___Amino Acid_________
5 ____Disaccharide___________
Draw an arrow to indicate the peptide bonds in the molecule below:
Explain how the two amino acids would join together to form a dipeptide and draw the final molecule.
H2O
Water is removed through dehydration synthesis and a bond is formed between the Carbon of the carboxyl
group and the nitrogen of the amino group
FINAL MOLECULE
Unit 2: Enzymes Review
1. What type of organic molecule is an enzyme? _______Protein_________
2. What is a catalyst and why is an enzyme considered a biological catalyst?
Catalysts speed up chemical reactions. Enzymes are made of proteins therefore they are considered
biological catalyst, unlike other catalyst such as heat.
3. Label enzyme activity below.
4. Describe the diagram above using the terms you used to fill in the diagram with.
The substrate will fit into the active site of the enzyme. The enzyme is able to lower the
activation energy of the reaction by various methods (stretching and bending bonds, creating a
microhabitat conducive for the reaction, holding the substrate close enough for the reaction to
take place and/or participating in the reaction). Once the reaction has taken place, the
products are released and the enzyme is free to catalyze another substrate reaction.
5. Answer true of false to the following statements:
a. ___T___ Enzymes interact with specific substrates
b. ___F___ Enzymes change shape after a reaction occurs
c. ___T___ Enzymes speed up reactions.
d. ___F___ One enzyme can be used for many different types of chemical reactions.
6. Circle the correct effect.
a. Raising the temperature slightly will _____________ the rate of reaction.
increase | decrease | not change If optimal temperature has been reached then it will
begin to decrease the reaction/enzyme activity rate due to the enzyme being denatured
b. Boiling temperature will _______________the rate of reaction.
increase | decrease | not change
c. Changing the pH toward the optimal pH will _____________the rate of reaction.
increase | decrease | not change
7. What four factors can affect the activity of an enzyme?
a. ___enzyme concentration___________
b. ___substrate concentration__________
c. ___temperature___________________
d. ____pH_________________________
Use the 2 graphs below to answer Questions 8, 9, and 10.
8. What is the optimal pH that this enzyme functions at? ________pH 8_________________
9. What is the optimal temperature that this enzyme functions at? ______35-40 oC________
10. What happens when the pH is 2?
The enzyme is denatured completely and will not function
11. Why are the active site and the substrates in an enzyme-catalyzed reaction often compared to
a lock and key?
The substrate must fit into the active site of the enzyme in order for the reaction to happen, just
like a key needs to fit into the lock correctly in order to function (lock or unlock door).