Replication, Transcription and Translation Honors Biology Powerpoint #2 – Chapter 12.
Honors Biology Chapter 2
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Transcript of Honors Biology Chapter 2
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Honors Biology Chapter 2
Chemistry
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DRY ERASE ATOM ATTITUDE
• Everyone gets a dry erase board, dry erase pen, and tissue for erasing.
• The teacher will ask you a question about atomic structure, you will write your answer and hold up your board.
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Are you wondering why we are learning chemistry in biology class?• All of our cells are made of chemical
compounds.
• All the activities of our bodies work on chemical reactions.
• All of our body’s reactions use water.
Such as neurotransmitters affecting neurons
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MATTER
• Anything that occupies space (VOLUME) and has MASS
• Is air matter?• Yes
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Match as energy (capacity to do work) or matter (occupies space
and has mass)
• Water• Electricity• Air• Helium• Sunlight• Iron• Carbon
• Matter• Energy• Matter• Matter• Energy• Matter• Matter
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2.1 ELEMENTS, ATOMS, 2.1 ELEMENTS, ATOMS, COMPOUNDS (are matter)COMPOUNDS (are matter)
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YOU NEED TO KNOW
• The Names (spelled correctly) and the Symbols (written correctly) on p. 18 (Table 2.1)
• “Elements in the Human Body”• 25 elements (includes trace
elements)• QUIZ on FRIDAY Sept. 27
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ELEMENTS
• Substance that cannot be broken down to other substances by ordinary chemical means (heating, adding an acid…)
• YouTube - ?Tom Lehrer's
The Elements" animated??
***ASAP SCIENCE Periodic Table
In Order
OR YouTube - ?The Elements Animation??
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Where can you find an element?
The Periodic Table of the Elements – see Appendix 2 and get your personal copy
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ELEMENTS AND SYMBOLS:Ca, H, Li, O, C, Mg
• What rules apply to writing the symbols (abbreviations of the elements)?
• First letter capital, second letter is lower case
• What are the four most common elements in the human body? (see chart)
• CHON• What are trace elements?• Less than 0.01% of human body weight
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Which are elements?
• Cu• C• CO• N• NO• WHY?• Cu C N only
one kind of matter Gold - Au
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COMPOUNDS• Substance of two or more different atoms chemically
combined in a fixed ratio• EXAMPLES: CO2
• H2SO4
• H2O
• CO• How is a compound written differently than an element?• More than one kind of element (more than one capital
letter).• NOTE: H2 is not a compound – its an element• (Only one kind of element)
Subscripts (tell how many atoms there are)
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Formula
• Formula is the abbreviation for a compound.
• CO2 H2SO4 H2O• Carbon dioxide sulfuric acid water• What rules seem to apply to writing a
formula?• Capital letters for elements• Subscript number behind and just below
the line of what element it represents
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Which are compounds?
• Na N H2 NO2 H2O Why?
• NO2
• H2O• 2 or more different elements
chemically joined (2+ diff. capital letters)
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Which are symbols?Abbreviations for elements
• C CO2 Mn CO Ni Why?
•C Mn Ni • Only one capital letter
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What’s the difference?
• Co CO co
• Symbol formula nothing
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Which are formulas?Abbreviation for a compound
• H2SO4 Cl2 H20 Al Why?
H2SO4 H20 abbreviations for compounds (2 or more different kinds of elements)
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Can you figure out the difference between a mixture and a
compound?
• A mixture is two or more elements (or compounds) NOT chemically joined.
• A compound is two or more atoms chemically joined.• Do Worksheet: Elements, Compounds, Mixtures
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DO WORKSHEET: Elements, Compounds, Mixtures
• (back of Atomic Mass and Atomic Number Worksheet)
• Work in groups of three, then we’ll compare answers.
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2.2 What are trace elements?• Needed in the body in only small
amounts• Like mg (milligrams)• WHY IMPORTANT IF WE DON’T
NEED SO MUCH?• Minerals act as catalysts (speed up
reactions) for many biological reactions
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Trace Elements
Needed by some organisms but only in very small amountsLike iodine, we need only 0.15 mg per dayA deficiency will cause a goiter
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Trace Elements
• Fluorine – in drinking water, toothpaste
• (help dental decay) But too much can cause fluorosis (white chalky build-up)
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Trace Elements
• Iron Rich Foods
• Most important
use is to carry
oxygen in the blood
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2.3 Atoms and Molecules
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Atoms are made of protons, neutrons, electrons
• Do you know what these particles are?
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Answers:
• Do you know what these particles are?
Protons
Neutrons
Electrons
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• Basic Atomic Structure Youtube (1:57)
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Atom
• Smallest unit of matter that retains the properties of the element
Li
Na
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Which shows one atom?
• C N N2 H20 Why?
• C and N • only one in number • Which are elements?• C N N2
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Molecule
• Two or more atoms held together by chemical bonds
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Which are molecules?
• Co CO CO2 O2
Why?
• CO CO2 O2 two or more atoms (alike or not alike, it doesn’t matter) bonded together
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Where is each subatomic particle located?
• Proton in the
• Neutron nucleus
Electron-outside the nucleus
• Golden Retrievers Show Atomic Structure Youtube (2:11)
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What is the charge of each subatomic particle?
• Proton Neutron Electron
• + O _• positive none negative
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What is the relative size?
• Proton neutron electron
• 1 amu 1 amu ~1/1836 amu• AMU = atomic mass unit = 1/12 CARBON ATOM• (standard)
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Neutral Atoms (no charge) (as seen on the periodic table)
• 39 Mass Number p + n K Symbol
• 19 Atomic Number p• (electrons = number of protons)• Neutral if negative charges = positive )
• n=mass no. – at.no.
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How can you tell the mass number and atomic number?
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When looking on the periodic table…
• Atomic Number• In order
• Identify element by its number of protons
• Mass Number• A decimal (average
of masses of all isotopes of that element)
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Why is the mass number a decimal?
Average of the Isotopes of Carbon• What is the mass
number decimal?• 12.011
• What would you round it to?
• 12
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What is the atomic number of?
• Silicon fluorine sodium WHY?
• 14 9 11• Number in succession (not
a decimal)• Number of protons
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What is the mass number of…?
• Carbon nitrogen hydrogen• WHY?
• 12 14 1• Decimal number on periodic
table• Not other number in succession• Number of p + n
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How do you find the number of…?• Protons electrons neutronsAtomic atomic mass number
number number minus atomic no.
(if neutral)
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How many?• Protons electrons neutrons
• Carbon
6 6 6
• Chlorine
• 17 17 18
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What is the atomic number?Mass Number?
• Number of p?
• Number of e-?
• Number of n?
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Do Atomic Mass and Atomic Number WORKSHEET
•Collaborate with your partner next to you, then we’ll see what’s right.
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ISOTOPES INTRO
• Isotopes (Virtual School) (2:51)
• Watch the video and list what facts you learned about isotopes.
• No, not about the Albuquerque Isotopes
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Isotope• Atoms that differ in number of neutrons• Also differ in mass number(since it is p + n)
• But all have the same number of protons
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Which is the most common isotope of Li? (check the
periodic table)
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Why is the Mass Number a Decimal?
• Finding the Average Atomic Mass (2:55)
• Watch this and find out how…
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How do you write chemical notation for isotopes?
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2.4 Radioactive Isotopes
• An isotope that decays spontaneously to emit (give off) particles or energy until it is stable
• Here a radioisotope is used to examine a thyroid gland
• Radioactive Tracers in Medicine (3:57)
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Radioactive Decay Examples
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Uses of Radioisotopes• C-14 dating (can date living things up to
6,000 years old) Carbon Dating (2:00 mins)
• Technetium 99 Radioisotope (2:58) • Nuclear Medicine: What to expect (2:46 mins)• Bozeman Biology Radioactive Dating (9 mins)• Carbon-14 Dating (2 mins)
Thyroid tumorHighlight parts of the body for diagnosis
PET SCAN: detect tumors, weak spots in arteries
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Uses of Radioisotopes
• Iodine-131 PIB molecule to
treat thyroid cancer detect Alzheimers
PET scan
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Negative Effects of Nuclear Radiation
• Chernobyl Nuclear Plant Accident
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Negative Effects of Radon
• Radon, a radioactive gas, causes lung cancer
• Found in regions containing uranium
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2.5-2.7 Chemical Bonds
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Ion• Charged atom
• Differs in number of electrons
• 39 Same mass number
K+ means lost one electron
• 19 Same atomic number
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ION
• Charged atom• Na+ (has lost one electron)• O-2 (has gained two electrons)• Shown with superscript +/- and
number on upper right• (can omit number if a “1”)• What's and Ion? Youtube (6:52)
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Ions form by gaining or losing electrons
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O-2 has gained two electrons
Na has lost an e- so it is Na+1
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Cation• Positive ion
• Na+
• Mg+2
• Lost electrons
Anion
• Negative ion
• Cl-
• O-2
• gained electrons
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If one electron is…
• Lost what charge will the ion have?
•+1
11p+11 e-
11p+10e-
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Which are ions?
• Cl O-2 Na+1 N2
Why?
• O-2 Na+1 • Charged atoms (lost or
gained electrons)• show charges as superscripts
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Valence Electrons
• Outer shell electrons
• Determines the bonding capacity of an atom
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How do electrons arrange themselves in an atom…
• In the outer electron shells (energy levels)?
• They are full with 2, 8, 8• Fill inner shell first, then go to next shell out(Outermost shell has the greatest energy)
Can you see any pattern how the e- arrange themselves?
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Get kinda complicated beyond 2,8,8…so that’s all we’ll do for now!
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Which electrons determine…
• The chemical properties of the atom?
• Outermost shell
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If one electron is gained…
• What charge will the ion have?
•-1
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• If 2 electrons are lost… What charge will the ion have?
•+2• If two electrons are gained…
What charge will the ion have?
•-2
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Filled outer e- shells
How many e- fill the first shell (nearest the nucleus)?How many e- fill the next two shells?
nucleus
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Gain 1 e- or lose 7 e-?
If gains 1 e-, then it becomes -1
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Gain 7 e- or lose 1 e-?
If loses 1 e-, the it becomes +1.
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Gain or Lose ?
If it could as easily lose or gain e-, then it will probably share them. It will form a covalent bond.
Tutorial 2.1 Chemical Bond Formation
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Fill in the chart of e-
Element Number of e-
First shell Second Third
Shell Shell
carbon 6
lithium 3
Sodium 11
Oxygen 16
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Fill in the chart of e-
Element Number of e-
First shell Second Third
Shell Shell
carbon 6 2 4
lithium 3 2 1
Sodium 11 2 8 1
Oxygen 8 2 6
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How are ion charges determined?• Cation = positive (+) ion
• Anion = negative (-) ion
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How are ion charges determined?
• If lose 1 e- = +1 charge
• If gain 1 e- = -1 charge
• If lose 2 e- = +2 charge
• If gain 2 e- = -2 charge
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Periodic Table Hint:
• You can tell how many electrons are in an atom’s outermost shell by just looking at its position on the periodic table!!!!!
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Note any pattern of valence electrons (outer shell) as they appear in the periodic table?
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+1 +2
share -3 -2 -1 0
e- in outer shells
Ion formed
e- in outer shell
Full outer e- shells
H
8
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How many electrons in each shell?(atomic number is given)
• Carbon oxygen fluorine sodium
• 12 16 9 11
• 2,4 2,6 2,7 2,8,1
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How many valence electrons?Will these atoms lose or gain e-
and how many?
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How many valence electrons?Will these atoms lose or gain e-
and how many?
Lose 1 lose O lose 1 share gain 3 lose 1
H+ He Li+ C N-3 Na+
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Now let’s do the Drawing Atoms Worksheet(and next 4 slides)
• How the electrons fill their shells (link)
• 1st shell – 1 pair• 2nd shell – e- space
far apart, singles, then pair
• 3rd shell – e- space far apart, singles, then pair
•
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Bohr Diagrams
C
1) Draw a nucleus with the element symbol inside.
2) Carbon is in the 2nd
period, so it has two energy levels, or shells.
3) Draw the shells around the nucleus.
![Page 90: Honors Biology Chapter 2](https://reader035.fdocuments.in/reader035/viewer/2022062321/56812c71550346895d910b14/html5/thumbnails/90.jpg)
Bohr DiagramLet’s do carbon (6 electrons)
• 1. Draw a nucleus.
• 2. Draw the number of rings needed.
• 3. Start in the first shell- only 2 e-, paired (put next to each other)
C
Get worksheet
![Page 91: Honors Biology Chapter 2](https://reader035.fdocuments.in/reader035/viewer/2022062321/56812c71550346895d910b14/html5/thumbnails/91.jpg)
Bohr Diagrams
1) Since you have 2 electrons already drawn, you need to add 4 more.
2) These go in the 2nd
shell.3) Add one at a time -
starting on the top and going counter clock-wise.
C
1
2
3
4
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Bohr Diagrams
If you were to have more electrons, start pairing them in the same clockwise order.
1
2
3
4
5
6
1
2
3
4
5
6
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Bohr model electron filling order
2
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Are these correct Bohr models?
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Are these correct Bohr models?
• What errors are at the ?
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Now do on the Atomic Structure Worksheet
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See the trend of how electrons fill the valence shells
• Lewis dot structures
• Octet Rule – electrons fill a shell until it’s full with 8 electrons
• Atoms are most stable with a filled outer electron shell
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What do we call the forces that…
• Hold atoms together in a molecule?
• Chemical bonds
• …not to be confused with James Bond
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Why do atoms bond?
•To have filled outer electron shells!
•Atom Heaven ATO
M
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What is a chemical bond?
• Attraction between two or more atoms YouTube - ?Ionic and covalent bonding animation??
![Page 101: Honors Biology Chapter 2](https://reader035.fdocuments.in/reader035/viewer/2022062321/56812c71550346895d910b14/html5/thumbnails/101.jpg)
Get Bonding Handouts
• Electronegativities
• Intermolecular Forces
• Bonding Reference Sheet
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Types of Bonds
Intramolecular
• Within the molecule
• -Ionic• -Covalent• Polar• Nonpolar
Intermolecular
• Between different molecules
• Van der Waals• London forces• Dipoles• Hydrogen Bonds
![Page 103: Honors Biology Chapter 2](https://reader035.fdocuments.in/reader035/viewer/2022062321/56812c71550346895d910b14/html5/thumbnails/103.jpg)
Bonding
• Covalent
• share electrons
• Ionic• transfer of
electrons
• (lose or gain)
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IONIC BOND
• lose one or more electrons become (+)
• gain one or more electrons become (-)
• The (+) and (-) ions formed now attract each other and form an ionic bond.
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Covalent Bonds
• Polar Covalent
• Unequal sharing of e-
• Nonpolar Covalent
• Equal sharing of e-
![Page 107: Honors Biology Chapter 2](https://reader035.fdocuments.in/reader035/viewer/2022062321/56812c71550346895d910b14/html5/thumbnails/107.jpg)
Covalent BondsClick HERE: Polar Covalent
Bonding (3 animations)•Electrons are shared
•Usually if near the same number of e- in outer shells
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Covalent bonding can be shown as:
• Bohr model
• Electron-dot
• Structural Formula
![Page 109: Honors Biology Chapter 2](https://reader035.fdocuments.in/reader035/viewer/2022062321/56812c71550346895d910b14/html5/thumbnails/109.jpg)
How can covalent bonds be written?
• Single bond double bond triple bond
• C-C C=C C=C• C:C C::C C:::C
• 2 e- 4 e- 6 e-
![Page 110: Honors Biology Chapter 2](https://reader035.fdocuments.in/reader035/viewer/2022062321/56812c71550346895d910b14/html5/thumbnails/110.jpg)
Writing Bonds• Each “ Each “ ––” ” is equal tois equal to
• “ “ :: “ or “ or
• ““two electronstwo electrons””
Single C – C or C:CDouble C = C or C::CTriple or C:::CC≡C
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Different Ways to Represent Four Common Molecules
butane
![Page 113: Honors Biology Chapter 2](https://reader035.fdocuments.in/reader035/viewer/2022062321/56812c71550346895d910b14/html5/thumbnails/113.jpg)
Making ionic bond in NaCl
• YouTube - ?Ionic and covalent bonding example??
• YouTube - ?Reaction of Sodium & Chlorine (with subtitles)??
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SALT =
• Synonym for an ionic compound
• Not just NaCl
Iron SulfideCopper Sulfate
Sodium chloride
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LET’S REVIEW: Which atoms combine…
• with other atoms?
• Ones that do not have filled outer electron shells
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REVIEW: What is the driving force to make atoms join with
other atoms to form compounds?
• TO HAVE FILLED OUTER ELECTRON SHELLS
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REVIEW: How does an atom…
• Get a filled outer electron shell?
• Gaining, losing, or sharing electrons
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What do you notice about the ion charge and the subscripts?
![Page 120: Honors Biology Chapter 2](https://reader035.fdocuments.in/reader035/viewer/2022062321/56812c71550346895d910b14/html5/thumbnails/120.jpg)
Do the Flip-Flop
• So you can cancel out the (+) and (-)
![Page 121: Honors Biology Chapter 2](https://reader035.fdocuments.in/reader035/viewer/2022062321/56812c71550346895d910b14/html5/thumbnails/121.jpg)
If there is only one atom, you do not need to write a “1”
You can reduce the subscripts if they are the same:
Fe+2 O-2 Fe2O2 reduce to FeO
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Electronegativity
•Get Electronegativities handout
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Electronegativity
Tendency of an atom to attract electrons towards itself and thusthe tendency to form negative ions.
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Electronegativity• The more electronegative
atom pulls shared electrons toward its nucleus.
• NONPOLAR – equal sharing of electrons
• POLAR – unequal sharing
of electrons
![Page 125: Honors Biology Chapter 2](https://reader035.fdocuments.in/reader035/viewer/2022062321/56812c71550346895d910b14/html5/thumbnails/125.jpg)
Electronegativities
• H = 2.1 O=3.5 C=2.5• H-H = 0.0 bond pure covalent• O-H bond = 1.4 polar • (3.5-2.1)• covalent• NaCl = 2.1 ionic
![Page 126: Honors Biology Chapter 2](https://reader035.fdocuments.in/reader035/viewer/2022062321/56812c71550346895d910b14/html5/thumbnails/126.jpg)
Molecule
• A group of two or more atoms held together by covalent bonds
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What’s the difference between Intramolecular
and Intermolecular Forces?
![Page 128: Honors Biology Chapter 2](https://reader035.fdocuments.in/reader035/viewer/2022062321/56812c71550346895d910b14/html5/thumbnails/128.jpg)
What’s the difference?• Intermolecular
attractions are between one molecule and a neighboring molecule
• (Van der Waals, hydrogen bonds)
• USUALLY WEAKER
• Intramolecular attractions are the forces which hold an individual molecule together (for example, the covalent bonds or ionic bonds).
• USUALLY STRONG
![Page 129: Honors Biology Chapter 2](https://reader035.fdocuments.in/reader035/viewer/2022062321/56812c71550346895d910b14/html5/thumbnails/129.jpg)
WHAT IS THE STRENGTH COMPARISON?
• STRONGEST BOND
• WEAKEST BOND
• Covalent
• Ionic
• Hydrogen
• Van der Waals• (dipole-dipole• London forces)
intramolecular
![Page 130: Honors Biology Chapter 2](https://reader035.fdocuments.in/reader035/viewer/2022062321/56812c71550346895d910b14/html5/thumbnails/130.jpg)
INTERMOLECULAR FORCES
• A. H-bonds (H to F, O, or N)
• B. van der Waals- temporary “dispersion” London (nonpolar) and dipole-dipole forces (polar)
• C. Disulfide bridges (-S-S-)• Intermolecular Forces Youtube (9:11-if ya got time)
•
![Page 131: Honors Biology Chapter 2](https://reader035.fdocuments.in/reader035/viewer/2022062321/56812c71550346895d910b14/html5/thumbnails/131.jpg)
• Intermolecular Forces
video and worksheet• What three types of intermolecular forces are there?• What does dipole mean? Why do those molecules
attract each other?• London forces are in molecules that are not dipoles.
What do they do to their e- to cause an attraction?• What three possible atoms can make a hydrogen bond
with hydrogen?• List the forces in order of strength.
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Hydrogen Bonds: Intermolecular between H and F, O, or N
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Where Might you find Hydrogen Bonds?
• In Water – between O- and H+
• In DNA – between bases
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Intramolecular: Van der Waals
• Van der Waals on Gecko Feet (8:22)
• Is the sum of the attractive forces between molecules (but not H-bonds or covalent bonds)
![Page 135: Honors Biology Chapter 2](https://reader035.fdocuments.in/reader035/viewer/2022062321/56812c71550346895d910b14/html5/thumbnails/135.jpg)
van der WaalsVan der Waals Dispersion Forces
•
Temporary dispersion of electrons make temporary charges
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Where might you find van der Waals?
• crystal structures (e. g. the shapes of snowflakes),
• DNA shape
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Intramolecular: (Van der Waal type) Dipole-dipole
• exists between neutral polar molecules only when they are close together
• Dipole Forces Bozeman youtube (7:32)• Temporary shift of the electrons to make a
partial + and a partial - end
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Weakest van der Waals:London Dispersion Forces
• Temporary polarity between nonpolar atoms or molecules
• All molecules have them at some time• Bozeman London Dispersion Forces (5:02)
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London Dispersion ForceLondon Dispersion Force Animation
![Page 140: Honors Biology Chapter 2](https://reader035.fdocuments.in/reader035/viewer/2022062321/56812c71550346895d910b14/html5/thumbnails/140.jpg)
Disulfide Bonds:Protein Tertiary Structure
• Disulfide Bond in Tertiary Protein
![Page 141: Honors Biology Chapter 2](https://reader035.fdocuments.in/reader035/viewer/2022062321/56812c71550346895d910b14/html5/thumbnails/141.jpg)
Disulfide Bonds
• formed between the side chains of cysteine in a protein SH) to form a disulfide bond (S-S)
• (Will learn about this in Chapter 3)
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THEME OF EMERGENT PROPERTIES
• New properties that arise with each step upward in the hierarchy or life, owing to the arrangement and interactions of parts as complexity increases.
• WHOLE IS GREATER THAN THE PARTS
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How is the emergent property idea apply to a compound and atoms?
• HINT:
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2.9 Chemical Reactions
• The making and breaking of chemical bonds, leading to changes in the composition of matter.
![Page 145: Honors Biology Chapter 2](https://reader035.fdocuments.in/reader035/viewer/2022062321/56812c71550346895d910b14/html5/thumbnails/145.jpg)
Chemical Reactions
• Reactants on the left of the arrow
• Products on the right of the arrow
• IDENTIFY:
• 2Mg(s) + O2(g) → 2MgO(s)
• MgO(s) + H2O(l) → Mg(OH)2(s)
• N2(g) + 3H2(g) → 2NH3(g)
![Page 146: Honors Biology Chapter 2](https://reader035.fdocuments.in/reader035/viewer/2022062321/56812c71550346895d910b14/html5/thumbnails/146.jpg)
Same number of each element on left side as on the right side
• CH4 (g) + 2O2 (g) CO2 (g) + 2H2O (g)
Reactants Products
C = 1
H = 4
O = 4
C = 1
H = 4
O = 4
![Page 147: Honors Biology Chapter 2](https://reader035.fdocuments.in/reader035/viewer/2022062321/56812c71550346895d910b14/html5/thumbnails/147.jpg)
Signs of a Chemical Reaction
• Precipitate forms
• Color Change
• Gas Forms
• Temperature change
![Page 148: Honors Biology Chapter 2](https://reader035.fdocuments.in/reader035/viewer/2022062321/56812c71550346895d910b14/html5/thumbnails/148.jpg)
Chemical Reaction Videos
• Na and Cl Chemical Rx (52 secs.)
• Genie in a Bottle Reaction - Steve Spangler (3:36)
• Weirdest Chem. Rx in the World (2:52) Mercury(II) thiocyanate Hg(SCN)2
• The Naked Scientists Videos (MP3)
![Page 149: Honors Biology Chapter 2](https://reader035.fdocuments.in/reader035/viewer/2022062321/56812c71550346895d910b14/html5/thumbnails/149.jpg)
Chemical Reaction Example
• An iron bar rusts. The iron reacts with oxygen in the air to make rust.
4 Fe + 3 O2 2 Fe2O3