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Name ___________________
Date ____________
CP Biology
Chapter 2 Study Guide – The Chemistry of Life
Read pages 34 – 37; 43-44; 50-51. TYPE the answer to the following questions
as you read each section. Write in complete sentences. Not all answers will be
found in the text; you might need to utilize the internet.
ATOMS
1. Define matter and atom.
2. Name the three subatomic particles and give the mass and charge
of each.
ELEMENTS AND ISOTOPES
1. Define element
2. Define atomic number and mass number of an atom.
3. Which four chemical elements are most abundant in living matter?
4. Define isotope.
Explain how radioactive isotopes differ from
isotopes.
5. Describe 2 biological uses for radioisotopes.
6. What are some potential risk factors of uncontrolled exposure to
radioisotopes?
CHEMICAL COMPOUNDS
1. Define compound.
2. In what ways do compounds differ from their component elements?
CHEMICAL BONDS
1. Define ion and ionic bonds. Give several examples of ionic
substances.
2. Define molecule and covalent bond. Give several examples of
covalent substances.
3. Explain how the valance electrons determine the chemical properties
of an atom.
4. What’s the maximum number of electrons that can be found in the 1st
energy level? The 2nd? The 3rd?
5. What determines whether atoms will form an ionic or covalent
bond?
ACIDS, BASES, and pH
1. What exactly does pH measure?
2. Define acid and base. Where do they fall on the pH scale?
3. Give examples of acids and bases.
4. What is a buffer and why is it important in biological systems?
CHEMICAL REACTIONS
1. What are reactants? What are products? Where are they found in a
chemical equation?
2. Since matter cannot be created nor destroyed, how are new
products formed during chemical reactions?
3. See the reaction in 2-19 (carbon dioxide in the bloodstream).
Name the reactants and the products.
Name __________________
Date __________
More Chemistry Review Fun!
(Yes, I’m sure you learned this already.)
Atomic Number = # of _______________
Mass Number= # of ___________ + # of ___________
Complete the table below.
Element
Symbol
Element
Name
Atomic
#
Atomic
Mass
# of
Protons
# of
Electrons
# Valence
electrons
# of
Neutrons
Net charge
on atom
C
H
O
N
Ca
Cl
Mg
Label the following parts of
the atom:
Nucleus
Electron
Proton
Neutron
Electron Cloud
trace element
radioisotope
ion
isotope
molecule
1. the substance formed when covalent bonds unite atoms
2. essential elements that are needed in small quantities
3. an atom that has gained or lost an electron
4. atoms of the same element, but different masses
5. unstable nucleus that emits energy and particles
6. The chart below shows the three isotopes of carbon. Some cells have been left blank. Apply
what you know about isotopes to fill in the blank cells.
Draw a Bohr Model of C-12, showing the
location of the protons, neutrons, and
electrons in their energy levels.
Isotopes of Carbon
Isotope
Number of
Protons
Number of
Electrons
Number of
Neutrons
Carbon–12
(nonradioactive)
Carbon–13
(nonradioactive)
6
6
6
Carbon–14
(radioactive)
7. Many of the molecules that make up living things are very large and complex. Water (H 2O) is
the most important small molecule in living things. Add two (small) atoms of hydrogen to the
oxygen atom below showing how they SHARE their valence electrons with oxygen to form 2
covalent bonds.
Oxygen
8. Below is the chemical equation for cellular respiration.
A) Balance the equation.
B) Label the reactants; label the products.
__C6H12O6 + __O2  __CO2 + __H2O + energy
C) Is cellular respiration endothermic or exothermic? ________________________
How do you know?
*Note- Each pH unit represents a 10x change in the concentration of H + in the solution.
9. On the pH scale above, write which direction is increasingly acidic and which is increasingly
basic.
10. Identify two solutions that have more H+ ions than OH– ions.
11. Identify two solutions that have more OH– ions than H+ ions.
12. How would you neutralize a solution that has a pH of 12?
13. What makes pure water neutral?
14. How many more H+ does pure water have than soap? ____________________
15. What is the concentration of hydrogen ions of normal rainfall? ______________