These exercises help to “cement” the informa????on in our brain so we can use that learning in our other tasks, both in life and in this course. When we exercise our thinking outside of reading and speaking, we can remember better and accomplish more.Instructions:
- Complete the tasks as outlined in the Biochemistry Worksheet (Word and PDF versions attached above for your convenience).
- Note: some tasks require that you draw from the Periodic Table of Elements, which is also attached above.
BIOCHEMISTRY Worksheet #1 (Module 2)
These exercises help to “cement” the information in our brain so we can use that learning in our other tasks, both in life and in this course. When we exercise our thinking outside of reading and speaking, we remember better and accomplish more.
Goal of this activity • To solve problems with atoms, molecules, and chemistry that are critical to maintaining life (biology)
Steps for Success with this activity 1. Look through the entire document, making note of what you have seen or heard previously. Rely on
your prior learning! Use that learning to build more. 2. Please remember that biology makes chemistry EASY! We learn applications of the chemical laws that
seem difficult. Actually, learning bio-chemistry will help you succeed in chemistry! 3. Work through the problems in any order.
a. Open the Periodic Table document. b. Typically the problems with the Periodic Table are important to understand prior to the work with
carbon molecules but do them in the order that makes sense to you. c. Sometimes starting with the last page will help you see the reason to learn the 1st page.
4. Work hard before you consult the answer page! Healthy frustration is the foundation of real learning, so let yourself be in a bit a “quandary” before you check your answers.
5. Bring all questions and inconsistencies to the Tech Live sessions.
TOPICS and ACTIVITIES A. Compare atoms, elements, chemical bonds, and molecules (OpenStax, Concepts of Biology, section 2.1)
1. Define: a) Matter = b) Elements = c) Atoms =
Application questions: Which of these groups have the largest number of members? Which of these are the smallest in size?
2. Within an ATOM, differentiate Elementary Particles (e.g., protons, neutrons, and electrons
Elementary Particle Charge Size (approximate) Location
Application questions: Which of these particles play a role in bonding? What is the job of the 3rd particle? When do we see that have an impact on an atom?
BIO 1000 – Module 2 Worksheet #1, page 2
3. Compare atomic bonds: ionic, covalent, and hydrogen-bonding (see OpenStax, Concepts of Biology, Figure 2.5, and extra practice sheet for electron dot diagrams)
BASIC RULE for CHEMICAL BONDING:
The goal of any bond is to be more STABLE (i.e. use less ENERGY).
This is described by the OCTET RULE.
STEP 1: How many electrons are in the outer orbit? (use the Periodic Table)
STEP 2: Determine if the outer shell is full.
Use the octet rule (except for Helium, on the top row). If the outer shell is FULL, it will neither accept any more electrons, nor will it give up any
electrons. COOL TRICK HERE: look at the Periodic Table.
• All of the atoms in the far-right column have FULL outer shells. (see column 18) • They are called “Noble Gases” for this reason; they do NOT react (e.g., form bonds)
under normal circumstances.
STEP 3: If the outer shell is not full, decide whether the electrons will be “stolen” or “shared”.
This depends how near the atoms are to one another on the Periodic Table. WHY?
We call this the difference in “electronegativity.” If the atoms are further apart on the Periodic Table, then the atom with an almost-full outer shell will be able “steal” another atom’s electron(s) from its almost-empty outer shell.
Opposite sides of the Periodic Table often means: LARGE or SMALL difference in electronegative. WHY?
STEP 4: Draw the compound, showing the shared or stolen electrons (see OpenStax, Concepts of Biology, Figure 2.5, and extra practice sheet for electron dot diagrams)
STEP 5: Determine the strength of the bond
If the electrons are “stolen,” the bond is IONIC, and easier to break. If the electrons are “shared,” then the bond is COVALENT and much more difficult to break.
Application questions: Which has a stronger bond? SODIUM CHLORIDE (NaCl) or METHANE (CH4)
Circle one; explain why this is true according to step 5.
ONE FINAL IDEA: After a molecule is formed, molecules are sometimes “pulled” toward each other.
Hydrogen bonds are one example of this type of association between different molecules. Water is one of the most famous examples of Hydrogen Bonding, shown in OpenStax,
Figure 2.7
BIO 1000 – Module 2 Worksheet #1, page 3
PRACTICE with drawing IONIC BONDING 1. Make an electron dot diagram of the atoms in the ionic compound. Check that your model is correct! 2. Draw the BEFORE model on this paper. Next, show IONIC BONDING by moving the valence electron(s). 3. Draw the AFTER model. Use arrows to show the electrons being transferred and indicate the charge of each atom.
PRACTICE with drawing COVALENT BONDING 1. Draw the electron dot diagrams of the atoms in each compound. RECOMMEND: use different colors for each atom
(or different “code”) 2. Then draw the line diagram to show each pair of shared electrons.
BIO 1000 – Module 2 Worksheet #1, page 4
Now that we have built the bonds, we can compare the bonds: ionic, covalent, and hydrogen-bonding.
Type of bond DEFINITION LOCATION of ELECTRONS STRENGTH IONIC
COVALENT
HYDROGEN- BONDING
B. Describe the properties of water that are critical to maintaining life
A. Water is a POLAR molecule due to its bond type. What does this mean? Draw it here (OpenStax, Fig. 2.7)
B. Because of its polarity, water has unique properties that support life on Earth. Name these properties of water:
1. _ 3. _
2. _ 4. _
C. Describe the ways in which carbon is critical to life
1. Life on Earth is also based on CARBON; often we call this “organic.”
2. A carbon atom can bond with 4 other atoms.
• Draw the simplest carbon molecule: Methane (CH4) (OpenStax, Fig. 2.13)
• Carbon can also make long-chain fatty acids; draw here. (OpenStax, Fig. 2.14)
D. Contrast the four major types of biological macromolecules and their functions
1. CARBOHYDRATES: made of , , and
• Always with a ratio of atoms at : : (such as glucose, C6H12O6)
2. LIPIDS include , , , , and
3. PROTEINS are made of individual parts called and have diverse functions.
4. NUCLEIC ACIDS include and . These are our genetic material (both genome and message).
- Goal of this activity
- Steps for Success with this activity
- TOPICS and ACTIVITIES
- BASIC RULE for CHEMICAL BONDING:
- PRACTICE with drawing IONIC BONDING
- PRACTICE with drawing COVALENT BONDING
,
BIOCHEMISTRY Worksheet #1 (Module 2)
These exercises help to “cement” the information in our brain so we can use that learning in our other tasks, both in life and in this course. When we exercise our thinking outside of reading and speaking, we remember better and accomplish more.
Goal of this activity
To solve problems with atoms, molecules, and chemistry that are critical to maintaining life (biology)
Steps for Success with this activity
1. Look through the entire document, making note of what you have seen or heard previously. Rely on your prior learning! Use that learning to build more.
2. Please remember that biology makes chemistry EASY! We learn applications of the chemical laws that seem difficult. Actually, learning bio-chemistry will help you succeed in chemistry!
3. Work through the problems in any order.
a. Have the Periodic Table document open as you work.
b. Typically, the problems with the Periodic Table are important to understand prior to the work with carbon molecules, but do them in the order that makes sense to you.
c. Sometimes starting with the last page will help you see the reason to learn the 1st page.
4. Healthy frustration is the foundation of real learning, so be patient with yourself and ask your professor if you have questions. Bring all questions and inconsistencies to the Tech Live sessions.
TOPICS and ACTIVITIES
Compare atoms, elements, chemical bonds, and molecules (OpenStax, Concepts of Biology, section 2.1)
1. Define the following terms:
a. Matter –
b. Elements –
c. Atoms –
2. Application questions for the above terms:
a. Which of these groups have the largest number of members?
b. Which of these are the smallest in size?
3. Within an ATOM, differentiate Elementary Particles (e.g., protons, neutrons, and electrons
|
Elementary Particle |
Charge |
Size (approximate) |
Location |
4. Application questions for the above table:
a. Which of these particles play a role in bonding?
b. What is the job of the 3rd particle? When do we see that have an impact on an atom?
5. Comparing atomic bonds: ionic, covalent, and hydrogen-bonding (see OpenStax, Concepts of Biology, Figure 2.5, and extra practice sheet for electron dot diagrams)
a. BASIC RULE for CHEMICAL BONDING:
· The goal of any bond is to be more STABLE (i.e. use less ENERGY).
· This is described by the OCTET RULE.
b. STEPS:
STEP 1: How many electrons are in the outer orbit? ( use the Periodic Table)
STEP 2: Determine if the outer shell is full.
· Use the octet rule (except for Helium, on the top row).
· If the outer shell is FULL, it will neither accept any more electrons, nor will it give up any electrons.
· COOL TRICK HERE: look at the Periodic Table.
· All of the atoms in the far-right column have FULL outer shells. (see column 18)
· They are called “Noble Gases” for this reason; they do NOT react (e.g., form bonds) under normal circumstances.
STEP 3: If the outer shell is not full, decide whether the electrons will be “stolen” or “shared”.
· This depends how near the atoms are to one another on the Periodic Table. WHY?
· We call this the difference in “electronegativity.” If the atoms are further apart on the Periodic Table, then the atom with an almost-full outer shell will be able “steal” another atom’s electron(s) from its almost-empty outer shell.
· Opposite sides of the Periodic Table often means: LARGE or SMALL difference in electronegative. WHY?
STEP 4: Draw the compound, showing the shared or stolen electrons (see OpenStax, Concepts of Biology, Figure 2.5, and extra practice sheet for electron dot diagrams)
STEP 5: Determine the strength of the bond
· If the electrons are “stolen,” the bond is IONIC, and easier to break.
· If the electrons are “shared,” then the bond is COVALENT and much more difficult to break.
c. Application questions:
· Which has a stronger bond? SODIUM CHLORIDE (NaCl) or METHANE (CH4) Circle or highlight the correct answer.
· Explain why the above is true, according to step 5.
d. ONE FINAL IDEA: After a molecule is formed, molecules are sometimes “pulled” toward each other.
· Hydrogen bonds are one example of this type of association between different molecules.
· Water is one of the most famous examples of Hydrogen Bonding, shown in OpenStax, Figure 2.7
PRACTICE with drawing IONIC BONDING
1. Make an electron dot diagram of the atoms in the ionic compound.
2. Draw the BEFORE model on this paper. Next, show IONIC BONDING by moving the valence electron(s).
3. Draw the AFTER model. Use arrows to show the electrons being transferred and indicate the charge of each atom.
PRACTICE with drawing COVALENT BONDING
1. Draw the electron dot diagrams of the atoms in each compound. RECOMMEND: use different colors for each atom (or different “code”)
2. Then draw the line diagram to show each pair of shared electrons.
( BIO 1000 – Module 2 ) ( Worksheet #1, page 2 )
Now that we have built the bonds, we can compare the bonds: ionic, covalent, and hydrogen-bonding.
|
Type of bond |
DEFINITION |
LOCATION of ELECTRONS |
STRENGTH |
|
IONIC |
|||
|
COVALENT |
|||
|
HYDROGEN- BONDING |
Describe the properties of water that are critical to maintaining life
1. Water is a POLAR molecule due to its bond type. What does this mean? Draw it below. ( OpenStax, Fig. 2.7)
2. Because of its polarity, water has unique properties that support life on Earth. Name these four (4) properties of water:
a.
b.
c.
d.
Describe the ways in which carbon is critical to life
Life on Earth is also based on CARBON; often we call this “organic.”
A carbon atom can bond with 4 other atoms.
1. Draw the simplest carbon molecule: Methane (CH4) ( OpenStax, Fig. 2.13)
2. Carbon can also make long-chain fatty acids; draw here. ( OpenStax, Fig. 2.14)
Contrast the four major types of biological macromolecules and their functions
1. CARBOHYDRATES are made of what three (3) things?
·
·
·
2. Always with a ratio of atoms at ____: ____: ____ (such as glucose, C6H12O6)
3. LIPIDS include the following things:
·
·
·
·
·
4. PROTEINS are made of individual parts called ________ _________ and have diverse functions.
5. NUCLEIC ACIDS include _______ and _______. These are our genetic material (both genome and message).
image1.png
image2.jpeg
,
PERIODIC TABLE OF ELEMENTS
Chemical Group Block
17Atomic Number
Cl Symbol
ChlorineName
Halogen Chemical Group Block
1
H Hydrogen
Nonmetal
1
1
2
He Helium
Noble Gas
18
3
Li Lithium
Alkali Metal
2
4
Be Beryllium
Alkaline Earth M…
2
5
B Boron
Metalloid
13
6
C Carbon
Nonmetal
14
7
N Nitrogen
Nonmetal
15
8
O Oxygen
Nonmetal
16
9
F Fluorine
Halogen
17
10
Ne Neon
Noble Gas
11
Na Sodium
Alkali Metal
3
12
Mg Magnesium
Alkaline Earth M…
13
Al Aluminum
Post-Transition …
14
Si Silicon
Metalloid
15
P Phosphorus
Nonmetal
16
S Sulfur
Nonmetal
17
Cl Chlorine
Halogen
18
Ar Argon
Noble Gas
19
K Potassium
Alkali Metal
4
20
Ca Calcium
Alkaline Earth M…
21
Sc Scandium
Transition Metal
3
22
Ti Titanium
Transition Metal
4
23
V Vanadium
Transition Metal
5
24
Cr Chromium
Transition Metal
6
25
Mn Manganese
Transition Metal
7
26
Fe Iron
Transition Metal
8
27
Co Cobalt
Transition Metal
9
28
Ni Nickel
Transition Metal
10
29
Cu Copper
Transition Metal
11
30
Zn Zinc
Transition Metal
12
31
Ga Gallium
Post-Transition …
32
Ge Germanium
Metalloid
33
As Arsenic
Metalloid
34
Se Selenium
Nonmetal
35
Br Bromine
Halogen
36
Kr Krypton
Noble Gas
37
Rb Rubidium
Alkali Metal
5
38
Sr Strontium
Alkaline Earth M…
39
Y Yttrium
Transition Metal
40
Zr Zirconium
Transition Metal
41
Nb Niobium
Transition Metal
42
Mo Molybdenum
Transition Metal
43
Tc Technetium
Transition Metal
44
Ru Ruthenium
Transition Metal
45
Rh Rhodium
Transition Metal
46
Pd Palladium
Transition Metal
47
Ag Silver
Transition Metal
48
Cd Cadmium
Transition Metal
49
In Indium
Post-Transition …
50
Sn Tin
Post-Transition …
51
Sb Antimony
Metalloid
52
Te Tellurium
Metalloid
53
I Iodine
Halogen
54
Xe Xenon
Noble Gas
55
Cs Cesium
Alkali Metal
6
56
Ba Barium
Alkaline Earth M…
57
La Lanthanum
Lanthanide
58
Ce Cerium
Lanthanide
59
Pr Praseodymium
Lanthanide
60
Nd Neodymium
Lanthanide
61
Pm Promethium
Lanthanide
62
Sm Samarium
Lanthanide
63
Eu Europium
Lanthanide
64
Gd Gadolinium
Lanthanide
65
Tb Terbium
Lanthanide
66
Dy Dysprosium
Lanthanide
67
Ho Holmium
Lanthanide
68
Er Erbium
Lanthanide
69
Tm Thulium
Lanthanide
70
Yb Ytterbium
Lanthanide
71
Lu Lutetium
Lanthanide
72
Hf Hafnium
Transition Metal
73
Ta Tantalum
Transition Metal
74
W Tungsten
Transition Metal
75
Re Rhenium
Transition Metal
76
Os Osmium
Transition Metal
77
Ir Iridium
Transition Metal
78
Pt Platinum
Transition Metal
79
Au Gold
Transition Metal
80
Hg Mercury
Transition Metal
81
Tl Thallium
Post-Transition …
82
Pb Lead
Post-Transition …
83
Bi Bismuth
Post-Transition …
84
Po Polonium
Metalloid
85
At Astatine
Halogen
86
Rn Radon
Noble Gas
87
Fr Francium
Alkali Metal
7
88
Ra Radium
Alkaline Earth M…
89
Ac Actinium
Actinide
90
Th Thorium
Actinide
91
Pa Protactinium
Actinide
92
U Uranium
Actinide
93
Np Neptunium
Actinide
94
Pu Plutonium
Actinide
95
Am Americium
Actinide
96
Cm Curium
Actinide
97
Bk Berkelium
Actinide
98
Cf Californium
Actinide
99
Es Einsteinium
Actinide
100
Fm Fermium
Actinide
101
Md Mendelevium
Actinide
102
No Nobelium
Actinide
103
Lr Lawrencium
Actinide
104
Rf Rutherfordium
Transition Metal
105
Db Dubnium
Transition Metal
106
Sg Seaborgium
Transition Metal
107
Bh Bohrium
Transition Metal
108
Hs Hassium
Transition Metal
109
Mt Meitnerium
Transition Metal
110
Ds Darmstadtium
Transition Metal
111
Rg Roentgenium
Transition Metal
112
Cn Copernicium
Transition Metal
113
Nh Nihonium
Post-Transition …
114
Fl Flerovium
Post-Transition …
115
Mc Moscovium
Post-Transition …
116
Lv Livermorium
Post-Transition …
117
Ts Tennessine
Halogen
118
Og Oganesson
Noble Gas
