Name __________________________________________ Period ___________ Date ________________
Ch. 2 Atomic Structure & Acid / Base Notes – part 1
Structure of Matter
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_____________________ - anything that takes up space and has mass (weight). It is composed
of elements.
____________________ - composed of chemically identical atoms:
o Bulk elements – required by the body in _________________ amounts
o Trace elements – required by the body in ________________ amounts
o Ultratrace elements – required by the body in very __________________ amounts
____________________ - smallest particle of an element
Elements and Atoms
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All matter is composed of ____________________
Elements are:
o Bulk elements
o Trace elements
o Ultratrace elements
Elements are composed of atoms of the __________________ type
Compounds are composed of atoms of different types that are ___________________________
Atomic Structure
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Atoms - composed of subatomic particles:
o Proton – carries a single ____________________ charge
o Neutron – carries __________ electrical charge
o Electron – carries a single ____________________ charge
Nucleus
o _________________ part of atom
o Composed of _____________________ and ___________________
o Electrons move around the nucleus
Label the Parts of the Atom and put the charges
Atomic Number and Atomic Weight
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Atomic Number
o Number of ___________________ in the nucleus of one atom
o Each element has a unique atomic number
o Equals the number of ________________________ in the atom
Atomic Weight
o Approximated by the number of _______________ plus the number of
_______________ in one atom (since a proton and a neutron each have an approximate
atomic weight of one)
o Electrons do not contribute to the weight of the atom
Isotopes
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Isotopes
o Atoms with the same atomic numbers but with different atomic ___________________
o Different numbers of _______________________
o Oxygen often forms isotopes (O16, O17, and O18)
o _______________________ isotopes are unstable, releasing energy or pieces of
themselves (atomic radiation)
For an element, the atomic weight is often considered the average of the atomic weights of its
isotopes.
Molecules and Compounds
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________________________ - particle formed when two or more atoms chemically combine
________________________ - particle formed when two or more atoms of different elements
chemically combine
_______________________ - depict the elements present and the number of each atom
present in the molecule
o Ex: H2
C6H12O6 H2O
Bonding of Atoms
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Bonds form when atoms combine with other atoms
Electrons of an atom occupy regions of space called
_______________________________lectron shells which circle the nucleus
For atoms with atomic numbers of 18 or less, the following rules apply:
o The first shell can hold up to ________ electrons
o The second shell can hold up to _________ electrons
o The third shell can hold up to ________ electrons
Bonding of Atoms: Ions
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Ion
o
o
Cation
o
o
Anion
o
o
An atom that ____________ or ______________ electrons to become stable
An electrically ____________________ atom
A ____________________ charged ion
Formed when an atom ________________ electrons
A ___________________ charged ion
Formed when an atom ____________________ electrons
Ionic Bonds
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Ionic bonds
o An attraction between a _____________________ and an ____________________
o Formed when electrons are __________________________ from one atom to another
atom
Covalent Bonds
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Formed when atoms ____________________ electrons
o Hydrogen atoms form ______________________ bonds
o Oxygen atoms form _________________ bonds
o Nitrogen atoms form ____________________ bonds
o Carbon atoms form _______________________ bonds
Bonding of Atoms: Polar Molecules
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Polar Molecules
o Molecule with a slightly ____________________ end and a slightly
__________________ end
o Results when electrons are not shared __________________ in covalent bonds
o _____________________ is an important polar molecule
Hydrogen Bonds
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Hydrogen bonds
o A ________________ attraction between the positive end of one polar molecule and
the negative end of another polar molecule
o Formed between ___________________ molecules
o Important for _____________________ and _________________________ structure
Chemical Reactions
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Chemical reactions occur when chemical bonds ________________ or ________________
among atoms, ions, or molecules
_____________________ are the starting materials of the reaction – the atoms, ions, or
molecules
_____________________ are the substances formed at the end of the chemical reaction
+
NaCl  Na + Cl
______________
-
______________
Bonding Worksheet
Acids, Bases, and Salts
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_______________________ - substances that release ions in water
o
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___________________ - electrolytes that dissociate to release hydrogen ions in water
o
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________________________________________
__________________ - substances that release ions that can combine with hydrogen ions
o
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________________________________________
________________________________________
__________________ - electrolytes formed by the reaction between an acid and a base
o
_______________________________________
Acid and Base Concentration
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____________________ - indicates the concentration of hydrogen in solution
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Neutral – pH ____________; indicates equal concentrations of ______ and ________
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Acidic – pH _______________________; indicates a greater concentration of H+
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Basic or alkaline – pH _____________________________; indicates a greater concentration of
OH-
Changes in pH and Buffers
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Blood pH
o
Normal blood pH is _________________________________
o
Alkalosis occurs when blood pH rises to 7.5 – 7.8
o
Acidosis occurs when blood pH drops to 7.0 – 7.3
o
_____________________________________mechanisms help regulate pH
o
Buffers are chemicals which act to _________________ pH change
Cabbage Juice Lab
Ch. 2 Biomolecules Notes – part 2
I.
What is a biomolecule?
II.
Organic molecules and Inorganic molecules—what’s the difference?
III.
Monomer and polymer—what’s the difference?
a. How are polymers formed?
b. How are polymers broken apart?
IV.
Carbohydrates:
a. Structure:
b. Function:
V.
Lipids:
a. Structure:
b. Function:
VI.
Proteins:
a. Structure:
b. Function:
VII.
Nucleic Acids:
a. Structure:
b. Function:
McMush Lab
Ch. 2 Enzymes Notes – part 3
1. Most enzymes are what type of macromolecule?
2. Most enzymes are ______________ or ______________ structures.
3. Enzymes act as ___________ in reactions.
4. Are enzymes permanently changed in the chemical reactions they are involved in?
5. Will an enzyme work on any substance? Explain.
6. Can enzymes be reused?
7. What ending is found on many enzymes?
8. Give 3 examples of enzymes with this ending.
9. How does an enzyme work?
10. What effect does an enzyme have on activation energy needed to start a reaction?
11. Hydrogen peroxide H2O2 is a common waste product of cells. Enzymes called catalases in cells break
this down into harmless ________________.
12. What is meant by the term substrate?
13. What is meant by active site?
14. Sketch and label the enzyme-substrate complex.
15. What is meant by induced fit?
16. What induces an enzyme to change the shape of its active site?
17. List 4 factors that can affect enzyme activity.
18. What is the effect of high temperature on an enzyme (running fever)?
19. What temperature do most enzymes do best at?
20. Most enzymes like a pH near ______________.
21. To denature an enzyme means the enzyme becomes _______________ and can no longer work
properly.
22. Name 3 inorganic substances (cofactors) that are often needed for enzymes to work properly.
23. Give an example of an enzyme & it’s needed inorganic substance.
24. Give one example of an enzyme inhibitor.
25. Explain how competitive inhibitors work.
26. If a competitive inhibitor blocks the active site, the ____________ can't fit.
27. Explain noncompetitive inhibitors.
28. Do noncompetitive inhibitors bind to the active site? Explain.
Toothpickase Lab