Transcript Atomic

Section 2.1
1. Atom:
the smallest unit of matter. Atoms consist of protons,
neutrons, and electrons.
2. Element:
One type of atom. It CAN NOT be broken down into a
simpler substance. It is a group of atoms of the same
type. What makes one element different from another
element? It’s # of proton’s!
3. Compound:
Is a substance made of atoms of different elements bonded together in
a certain ratio. Example: H20
Atomic Model
Proton: a very small particle of
matter that is part of the nucleus of an
atom and that has a positive
electrical charge
Neutron: a very small particle of
matter that has no electrical charge
and is part of the nucleus of all atoms except hydrogen atoms
Electron: a very small particle of matter that has a negative charge of electricity and
that travels around the nucleus of an atom
Isotopes: atoms of the same element with different # of neutrons.
Your # of protons & electrons in an atom are equal
6
6
C
12
C
13
Bohr’s Atomic Model
Page 35 in textbook
First Shell holds 2 Electrons
Second Shell holds 8 Electrons
Third Shell holds 8 Electrons
Fourth Shell holds 18 Electrons
Fifth Shell holds 18 electrons
Six Shell holds 32 Electrons
10
Ne
20
# of total electrons
Scientist Bohr: depicts the atom as a small,
positively charged nucleus surrounded by
electrons that travel in circular orbits around
the nucleus
View Atomic Model
Atomic #
Equals #
of protons
With a partner (using a laptop)
Create atoms for 10 elements
Atomic Mass:
Equals # of protons
plus number of
neutrons
17
Cl
Chlorine
35.45
When creating atoms:
1. Look at the atomic # - that will tell you how many protons you have
2. Look at the atomic mass, Subtract the Atomic # from the Atomic Mass and that
will tell you how many neutrons you have!
3. You have the same # of electrons as protons. You just need to correctly fill each
shell! If you forget how many electrons are in each shell, reference your periodic
table!
Section 2.1
4. Ion: Is an atom that has gained or lost one or more
electrons in it’s outer valence shell.
5. Ionic Bond: A bond where you lose or gain an
electron.
(Ionic Bond View with Covalent Bond animation)
6. Covalent Bond: A bond where atoms share a pair of
electrons
Covalent Bond
Covalent Bond
7. Molecule: Two or more atoms held together by
covalent bonds.
Example: Co2 Carbon and Oxygen SHARE the
electrons in the outer shell.
Section 2.1
11
Na
22
NA
17
Cl
# of electrons
Cl
Mass of Na is 22g, loses a electron so now more positive.
Cl gains an electron so becomes more negative!
**Remember electrons have a negative charge**
Take out your Periodic table: Label
Section 2.1
Take out your Periodic table:
Complete the following Chemistry Worksheet
First, write the COMPOUND product you would receive when combining the two
elements.
Second, draw the Lewis dot representation of the ionic bonding that is occurring.
** Remember Ionic bonding means you gain or lose an electron.**
Example:
One Carbon plus one Hydrogen equals
Carbon- 4 e outer shell, and 2 in inner shell
6
1
C
H
H
C-4 H+1 = CH
4
Every bond/line equals
2 electrons
H
C
H
H
H
H
C
H
H
Section 2.3
Organic Chemistry
All about the Element Carbon
Carbon atoms have four electrons in their outer shells, and all four are
available for bonding. Carbon can share these electrons in single bonds with
up to four other atoms to form very stable structures.
C
Carbon can form multiple bonds with up to two other atoms by sharing two
or more electrons with another atom; forming double bonds or even triple
bonds!
Carbons ability to form four bonds in a single plane makes it uniquely suited
to form macromolecules.
1 line equals 2 electrons
Carbon can also readily form bonds with other carbon
atoms to form long, complex molecules. When chemists
refer to organic molecules, they generally use structural
formulas. A diagram of the molecule is often more helpful
than the name. Because of the high percentage of carbon
and hydrogen in organic molecules, the molecules are
drawn without labeling them. Carbon atoms are located
where lines intersect, unless otherwise noted, and the 4
bonds around each carbon are understood to be completed
by the appropriate number of hydrogens.
Below are examples of some common carbon-containing
compounds.
Section 2.3
Biological Molecules
Biological molecules are composed of small repeating
subunits that bond together to form larger units. The
subunits, or building blocks, are called monomers.
Polymers are the complex molecules formed from the
repeating subunits.
There are four basic classes of complex organic molecules,
or macromolecules, that compose cells: carbohydrates,
proteins, lipids, and nucleic acids
Section 2.3
Carbohydrates
Carbohydrates are organic macromolecules that are made
up of carbon, hydrogen, and oxygen atoms. These atoms
are combined in a ratio of:
1 carbon atom : 2 hydrogen atoms : 1 oxygen atom
The presence of multiple carbon-hydrogen bonds within
carbohydrates makes them an excellent source of energy
Carbohydrates may be simple or complex.
The building blocks of carbohydrates are the simple sugars
known as monosaccharides. Sugars such as glucose,
fructose, and ribose are all examples of monosaccharides.
Monosaccharides can be combined to form more complex
carbohydrates known as polysaccharides. Glycogen,
starch, and cellulose are all examples of polysaccharides.
Glucose
Starch
Section 2.3
Lipids
Lipids are organic macromolecules that are insoluble in
water. This is why lipids are often found in biological
membranes and other waterproof coverings (e.g. plasma
membrane, intracellular membranes of organelles). These
lipids play a vital role in regulating which substances can or
cannot enter the cell.
The most important lipids, however, are fats. Triglycerides
are a type of fat that contain one glycerol molecule and
three fatty acids.
Section 2.3
Lipids
Fatty acids are long chains of CH2 units joined together.
The fatty acids in saturated fats do not contain any double
bonds between the CH2 units whereas the fatty acids in
unsaturated fats contain some carbon-carbon double
bonds. Saturated fats are found in butter, cheese,
chocolate, beef, and coconut oil. Unsaturated fats are
found in olives and olive oil, peanuts and peanut oil, fish,
and mayonnaise.
Fats are important because they are a major source of
energy. Since they contain even more carbon-hydrogen
bonds than carbohydrates, fatty tissue has the ability to
store energy for extended periods of time
Unsaturated means containing a carbon double or triple
bond.
Section 2.3
Proteins
Proteins are organic macromolecules that are composed of amino acid monomers.
There are 20 essential amino acids that are used by all living things to construct
proteins. These amino acids are made up of the elements carbon, hydrogen, oxygen,
and nitrogen. Some of the amino acids also contain sulfur. Three of the amino acids
are shown below.
There are three main
components of an amino acid,
shown to the left.
Proteins differ from each other due to the number and arrangement
of their component amino acids. Proteins also take on unique
shapes as determined by their amino acid sequences.
Proteins are different then Carbohydrates because they can catalyze
biochemical reactions.
(Enzymes are proteins)
Section 2.3
Carbohydrates vs. Proteins
• Proteins are made up of the elements
C,H,O, and N while Carbohydrates only
contain C,H, and O (elemental ratio of
these three is 1:2:1)
Carbohydrate
Protein
Carbohydrates vs. Proteins
Functions
• Carbohydrates are our essential energy
molecules to be use almost immediately
(simple sugars like glucose) or stored in
the liver as glycogen.
• Proteins are building and regulatory
compounds (such as hormones and
enzymes). Muscles and cell membranes
contain proteins
(why weight lifters eat a lot of protein)
Section 2.3
Nucleic Acids
Nucleic acids are formed from nucleotide monomers. Nucleotides are chemical
compounds that are primarily comprised of the elements carbon, hydrogen, oxygen,
nitrogen, and phosphorus. They consist of a five-carbon sugar, a nitrogenous
base, and one or more phosphate groups.
There are two main types of nucleic acids - ribonucleic acids (RNA) and
deoxyribonucleic acids (DNA). These nucleic acids are different because their fivecarbon sugars are different. RNA contains ribose, and DNA contains deoxyribose.
There are five nitrogenous bases found in nucleic acids.
Adenine (A), cytosine (C), and guanine (G) are found
in both DNA and RNA. Thymine (T) is only found in
DNA, and uracil (U) is only found in RNA.
Section 2.3
1. Monomer: molecular subunit of a polymer
2. Polymer: large carbon based molecule formed by
monomers.
3. Carbohydrate: molecule composed of carbon,
hydrogen, and oxygen; including sugars and starches.
4. Lipid: nonpolar molecular composed of carbon,
hydrogen, and oxygen; includes fats and oils.
Section 2.3
1. Fatty Acid: hydrocarbon chain often bonded to glycerol in a
lipid.
A triglyceride is three fatty acids and a glycerol.
The red portion of the diagram is one glycerol. Each black
chain is a fatty acid.
1. Protein: polymer composed of amino acids linked to
peptide bonds, Any of a group of complex organic
macromolecules that contain carbon, hydrogen, oxygen,
nitrogen, and usually sulfur and are composed of one or
more chains of amino acids
2. Amino Acid: Molecule that makes up proteins; composed
of carbon, hydrogen, oxygen, nitrogen, and sometimes
sulfur, building blocks of proteins.
3. Nucleic Acid: polymer of nucleotides; the genetic material
of organisms, carries genetic information directing all
cellular functions DNA.
Dalton’s Atomic Theory
The main points of Dalton's atomic theory were:
• Elements are made of extremely small particles called
atoms.
• Atoms of a given element are identical in size, mass, and
other properties; atoms of different elements differ in size,
mass, and other properties.
• Atoms cannot be subdivided, created, or destroyed.
• Atoms of different elements combine in simple wholenumber ratios to form chemical compounds.
• In chemical reactions, atoms are combined, separated, or
rearranged.
Dalton’s Atomic Theory
Law of Conservation of Mass: No detectable gain or loss of
mass occurs in chemical reactions. Mass is conserved.
This is why all chemical reactions are balanced on both sides
Example:
2C4H10 + 13O2  8CO2 + 10H2O
C= 8
C=8
H=10
H=10
O=26
O=26
Law of Definite Proportions: In a given chemical compound,
the elements are always combined in the same proportions by
mass.
Example: H2O always 2 H’s to every 1 O
How many atoms of each element are in the formulas?
C-4 H+1 = CH4
1. Al2 (SO4)3
Al=2 S= 3 O=12
2. CoCl3 ·6H2O
Co= 1
H=12
Chemical Equation
Zn + S

ZnS
ReactantsProduct
** No gain or loss of mass occurs in chemical reactions**
** Manipulate Coefficients to make an equation conform to the
law of conservation of mass**
Example:
2
Mg (OH)2 + 2HCL  MgCL2 __H2O
Mg=1 H=4
Mg=1
Cl=2
Cl=2 Need 2 H and a O
O=2
H=2 O=1
Section 2.2
Periodic Table
1. Hydrogen Bond:
a weak chemical bond between an electronegative atom, such
as fluorine, oxygen, or nitrogen, and a hydrogen atom bound to
another electronegative atom.
2. Cohesion:
is the property of like molecules (of the same substance) to
stick to each other due to mutual attraction. Ex: H2O molecules
sticking together
3. Adhesion:
is the property of different molecules or surfaces to cling to
each other. Example: H2O in a tube creating a meniscus
4.Solution:
A homogeneous mixture of two or more substances
Section 2.2
1. Solvent:
the liquid in which a solute is dissolved to form a solution.
2. Solute:
the substance dissolved in a given solution
3. Acid:
Substance that donates hydrogen ions. Has a pH of less than
7.
4. Base: A substance that accepts hydrogen ions, has a ph
between 7 and 14.
5. PH: How Acidity and alkalinity are measured.
Section 2.4
1. Chemical Reaction: a process that involves changes in the
structure and energy content of atoms, molecules, or ions.
2. Reactant: The substance that is present at the start of the
reaction. Also is the substance that is changed during the
chemical reaction.
3. Product: A substance resulting from a chemical reaction.
4. Bond Energy: measure of strength in a chemical bond. The
amount of energy it will take to break a bond between two
atoms.
Page 51 in textbook
Section 2.4
1. Equilibrium: when both the reactants and products are
made at the same rate.
2. Activation Energy: Is the amount of energy that needs to
be absorbed for a chemical reaction to start.
Releases
energy!
Add H2O reaction occurs
Energy is transferred through heat
and light
1. Exothermic: Chemical reaction releases more energy than
it absorbs. If the products have a lower bond energy than
the reactants, the reaction is exothermic.
2.Endothermic: Chemical Reaction absorbs more energy
than it releases. If products have a higher bond energy than
reactants, the reaction is endothermic.
When trying to classify a process as exothermic or endothermic, watch how the
temperature of the surroundings changes. An exothermic process releases heat,
and causes the temperature of the immediate surroundings to rise. An endothermic
process absorbs heat and cools the surroundings.
Examples:
Exothermic- Making ice cubes
Endothermic-melting ice cubes
Section 2.5
1. Catalyst:
substance that causes or accelerates a chemical reaction
without itself being affected.
2. Enzyme:
a substance produced by a living organism that acts as
catalyst to bring about a specific biochemical reaction.
3. Substrate:
Is the material on which an enzyme acts on. It is the reactant
that binds to the catalyst.
ALL MADE OF ATOMS
_______________________
MATTER
•The smallest basic unit of _______________
•Consist of three types of smaller particles:
Positive Charge
PROTONS
•________________________________________
NEUTRONS
No Charge
•________________________________________
ELECTRONS
Negative Charge
•_________________________________________
ELECTRONS
PROTONS
________________
________________
NEUTRONS
_________________
ATOM
•One type of _______________
•Cannot be _________
BROKEN _______
DOWN into a simpler substance.
•Examples:
Gases
HYDROGEN
________________
Metals
ALUMINUM
________________
OXYGEN
________________
GOLD
________________
What makes one element different from another?
The number of PROTONS
________________________
•A SUBSTANCE MADE OF ATOMS(OR ______________)
ELEMENTS
THAT ARE _____________
TOGETHER IN A CERTAIN
BONDED
RATIO.
•EXAMPLES
WATER ( H2O )
________________
CARBON
DIOXIDE ( CO2 )
_______________________
GAINED OR ___________
LOST
• AN ATOM THAT HAS ___________
ONE OR
MORE ELECTRONS.
•ATOMS BECOME IONS WHEN THEIR
NUMBER OF ELECTRONS IS CHANGED
______________________________________________
LOSE
•POSITIVELY CHARGED IONS – ________
ELECTRONS
GAIN ELECTRONS
•NEGATIVELY CHARGED IONS – _______
•IONS FORM BECAUSE ATOMS ARE MORE STABLE WHEN
OUTERMOST ENERGY LEVEL IS _______.
FULL
THEIR _____________
POSITIVELY CHARGED
•________________________
IONS ARE ATTRACTED TO
NEGATIVELY CHARGED
_________________________
IONS
The sodium atom loses its one
outer electron to the chlorine atom.
Na loses an electron to Cl
The positive sodium ion and
negative chloride ion attract each
other and form an ionic bond.
Gained electron
Ionic bond
Sodium atom (Na)
Chlorine atom (Cl)
IONIC BONDS
___________________________:
OPPOSITELY CHARGED IONS.
Sodium atom Chlorine atom
(Na+)
(Cl-)
ELECTRICAL FORCE BETWEEN
FORM THROUGH THE ____________________________
COVALENT _______.
BONDS
•Two or more atoms held together by __________
ELEMENT
•Smallest part of a ____________________.
•Almost all substances that make up organisms,
LIPIDS, NUCLEIC ACIDS, WATER
(____________________________________________)
are
molecules held together by covalent bonds.
covalent bonds
CARBON DIOXIDE (CO2):
Oxygen:
_____Protons,
8
___
8 Neutrons
_____Electrons
(6 outer/2 inner)
8
6
C
6
6 Neutrons 12
_____Protons,
___
_____Electrons
(4 outer/2 inner)
6
Carbon:
Oxygen Atom (O) Carbon Atom (C) Oxygen Atom (O)
COMPOUND:
WATER = H2O
= OXYGEN
= HYDROGEN
7
MOLECULES OF H2O = ______
Practice:
How many water molecules will be
created as a result of covalent bonds?
= OXYGEN
= HYDROGEN
“EXTRA” ELEMENTS
TOTAL MOLECULES OF WATER
OXYGEN
7
___________
2
___________
HYDROGEN
1
___________
More Practice:
How many water molecules will be
created as a result of covalent bonds?
= OXYGEN
= HYDROGEN
“EXTRA” ELEMENTS
TOTAL MOLECULES OF WATER
OXYGEN
11
___________
0
___________
HYDROGEN
4
___________
1. Matter:
Anything that has mass and takes up space.
Made up of atoms.
2. Atoms:
Make up elements
3. Elements:
Substances that are made up of only one kind of atom
oxygen, hydrogen, carbon, nitrogen
4. Compound: Substances that are made up of two or more elements
Water, (H2O) , Carbon Dioxide, (CO2)
5. Molecule: The smallest part of a compound
You must have 2 hydrogen molecules and 1 oxygen to have WATER.
__________________________________________
OXYGEN,
(O)
____________
____________
CARBON,
(C)
____________(H)
HYDROGEN,
____________
NITROGEN, (N)
____________
CALCIUM,
(Ca)
____________(P)
PHOSPHORUS,
_OTHER_____
____________
SULFUR,
(S)
CELLS
•Organisms’ bodies, (their _____________),
WATER
are made up of mostly ____________________
STRUCTURE
•The water in cells gives the cell _______________
TRANSPORTS
and ___________________
materials within
organisms.
•All of the processes necessary for an
organism’s life take place within the
WATERY ENVIRONMENT of the cell
______________________________
______________________
1. HIGH
SPECIFIC HEAT
______________________
2. COHESION
______________________
3. ADHESION
Negative Charge
POLAR
•Water is a “______________”
molecule
•Form when atoms in a molecule
UNEQUAL pulls on the
have ____________
ELECTRONS
_____________ they share.
Positive Charge
•Opposite charges of polar molecules can
HYDROGEN
interact to form ____________________
bonds.
•An attraction between a slightly
POSITIVE
_______________
hydrogen atom
and a slightly ______________
NEGATIVE
atom.
(Usually
_______________________________)
OXYGEN OR NITROGEN
•Hydrogen bonds are part of the
PROTEINS
structures of _______________
and
of ______________
DNA
Positive Charge
Shared Electrons
HIGH SPECIFIC HEAT
• Hydrogen bonds give water an abnormally ____________________________.
RESISTS
•Water __________________
changes in temperature because it must
_____________
____________________ to increase in temperature.
absorb more more
heat energy
Cohesion: the attraction among
__________________
of the same
MOLECULES
substance.
Cohesion from hydrogen bonds makes
water molecules _____________________.
STICK TOGETHER
Cohesion produces __________________,
SURFACE TENSION
( “skin on water” )
Adhesion: the attraction among
__________________
MOLECULES of ______________
DIFFERENT
substances.
For example, water molecules stick to other
things.
Water in a test tube, (water is attracted
to the ____________)
GLASS
Materials such as
SUGARS
________________
and
____________
cannot be
OXYGEN
transported form one part
of an organism to another
unless they are dissolved
in blood, plant sap, or
other water based fluids.
SOLUTION
______________:
Mixture of a substance
that is the same
throughout.
SOLVENT
___________:
Substance that is present
in the greater amount and
dissolves another
substance.
SOLUTE
___________:
Substance that dissolves
in a solvent.
ACIDS
BASES
Some compounds form ______________
or _____________
BREAK UP
IONS
because they _______________
into _______________
WATER
when they dissolve in ___________.
BASE:
ACID:
Compounds
that release
a proton
- a hydrogen ion(H+) –
when it dissolves
in water
Compounds that
remove H+ ions
from
a solution
PROTEIN
____________________
LIPIDS
____________________
CARBOHYDRATES
____________________
ATP
____________________
NUCLEIC ACID
____________________
•USED BY CELLS FOR __________
ENERGY ___________
SOURCE
AND
__________
ENERGY____________.
STORAGE
SIMPLE CARBS = _______________________________
ONE OR TWO SUGAR MOLECULES
COMPLEX CARBS =LONG
_____________________________
CHAINS OF SUGAR
MOLECULES
_____________________________
Ex) Starches such as potato,
________________________________
pasta, bread
________________________________
CELLS
•MAKE UP _________________.
LIFE PROCESSES
•INVOLVED IN ALL _______
____________.
AMINO ACIDS
•BUILDING BLOCKS = _________
__________.
ENZYME
•_________________=
TYPE OF PROTEIN THAT STARTS
AND SPEEDS UP CHEMICAL REACTIONS IN CELLS.
WATER
•DON’T MIX WITH ______________.
CELL MEMBRANE
•PHOSPHOLIPIDS – MAKE UP ________
______________.
STORE___________.
ENERGY
•FATS AND OILS THAT _________
•ORGANISMS USE FATS AND OILS WHEN THEY HAVE
CARBOHYDRATES
USED UP ___________________.
FATS
•_________SOLID AT ROOM TEMPERATURE.
OILS
•_________LIQUID AT ROOM TEMPERATURE.
ENERGY CARRYING
•MAJOR ___________
___________ MOLECULE IN CELL.
CARBOHYDRATES AND __________
LIPIDS
•ENERGY IN __________________
AND
PROTEINS
_____________________
MUST BE TRANSFERRED TO
ATP IN CELL TO BE USED.
PROTEIN
•HAVE ALL INFO NEEDED TO MAKE __________.
BLUE PRINT
•“_______________”
OF LIFE.
•BUILDING BLOCKS OF NUCLEOTIDES
_____________.
DNA
RNA
•TWO TYPES: ________
AND _______.
COMPOUND
BUILDING BLOCK
(POLYMER)
(MONOMER)
PROTEIN
AMINO ACID
LIPID (FAT)
FATTY ACID
CARBOHYDRATE
SUGARS
NUCLEIC ACIDS
NUCLEOTIDE