A&P Chapter 2: The Chemistry of Life

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Biology

•

11th Grade

•

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Joseph Beshara

Used 3+ times

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49 Slides • 66 Questions

Chapter 2

Chemistry of Life

• Matter -Anything that occupies space and has mass

• Atoms- basic units of matter

• Element -Pure substance. Made of only 1 type of atom.
Example: A bar of iron (Fe) is made of only iron atoms

•

• Molecules - particle of matter made of more than 1 type of atom
EXAMPLE Water (H₂O) is made of hydrogen atoms and oxygen atoms.

Chemical Level of Organization

⬤ Nucleus: The center of the atom

� Proton: Has a positive charge. In nucleus.

� Neutron: Has a neutral (0) charge. In nucleus

� Atomic number: Number of

protons in the nucleus
Atomic number tells you the name of the element

� Atomic mass: Number of

protons plus neutrons
Also called the MASS number
MASS NUMBER = # of protons + # of neutrons

Structure of an Atom: The

Multiple Choice

Anything that takes up space and has mass is called...

atoms

matter

element

molecule

Multiple Choice

CHOOSE THE BEST ANSWER: Proteins are made of many Nitrogen, Oxygen, Carbon, and Hydrogen Atoms. This is an example of an.....

Matter

Atoms

Element

Molecule

Multiple Choice

CHOOSE THE BEST ANSWER: An aluminum can is made of only aluminum atoms. This is an example of a/an

Matter

Atoms

Element

Molecule

Multiple Choice

The center of an atom is called the________________

Energy levels

electrons

nucleus

atomic number

Multiple Select

Pick all that apply: In the nucleus _______________ can be found

Protons

electrons

neutrons

energy levels

Multiple Select

Pick all that apply: The atomic number tells you what 2 things?

Name of the element

How many protons

How many neutrons

energy levels

Multiple Choice

Which element has an atomic number 17?

Carbon

oxygen

chlorine

fluorine

Multiple Choice

Antimony (Sb) has an atomic number of _____

121.76

118.81

Multiple Choice

An atom has a mass number of 20 and 10 protons. How many neutrons does this element have?

Multiple Choice

An atom has a mass number of 16 and 8 neutrons. What is the name of the element?

chlorine

Chromium

oxygen

nitrogen

Multiple Choice

An atom as an atomic number of 12. This element also has 12 neutrons. What is its mass number? (HINT: What does atomic number tell you?)

Multiple Choice

How many protons does Gold (Au) have?

Fill in the Blanks

⬤
Energy levels: Orbits around the nucleus. Contains Electrons

� Electron: has a negative charge

� Each energy level may contain a different number of electrons

� Number of electrons in outer energy level determines chemical

behavior

Energy Levels

Model of an Atom

Match

Match each type of charge with the subatomic particle

Negative charge

positive charge

no charge or neutral

electrons

protons

neutron

Multiple Choice

Which of these is the proton.

None

Multiple Choice

Which of these is the electron?

⬤ Molecule: Larger chemical unit of atoms

⬤ Element: Pure substance;

composed of only one element.
Sometimes can be a molecular element
The "gens": Oxygen (O2) Hydrogen (H2), Nitrogen (N2) Halogen (X2)

⬤ Compound:

2 or more different elements

⬤ Chemical formula determines atoms present in a

compound

Elements, Molecules, and

Compounds

Categorize

Options (6)

A bar of Pure Gold

Chlorine (a halogen)

Table Salt (NaCl)

Table sugar (C12H24O11)

Hydrochloric Acid (HCl)

Sort between an element or a compound

Element

Compound

⬤ Isotope: Same element with a different number of neutrons

⬤ Radioactive isotope: Isotope that emits radiation

� Sometimes used in nuclear medicine to evaluate the

function of body parts

⬤ Exposure to high radiation levels may cause cancer

cells to develop

Radioactive Isotopes

Multiple Choice

The same element with two different masses is called a/an...

isomer

molecule

isotope

ion

Types of Bonds

⬤ Chemical bonds form to make atoms more stable

� Stability occurs when outermost energy level of each

atom becomes full

⬤ Two types of chemical bonds we will examine:

Ionic bonds

• Between METAL and NON METALS

• electrons are TRANSFERRED

• Ex: Table Salt is Sodium Chloride (NaCl)

Covalent bonds – Covalent means sharing

• Between NON METALS

• Electrons are shared

• EX: Water (H₂O) and Carbon Dioxide (CO₂)

Chemical Bonding

To see what is metal or nonmetal:Find the steps.

Left of the Steps:
METALS
Right of steps
NONMETALS
The steps are
called metalloids
The only
exception is
Hydrogen (it is
non metal)

Metals vs Nonmetals

Categorize

Options (16)

Chlorine (Cl)

oxygen

Carbon

Hydrogen

Sodium (Na)

Iron (Fe)

Nitrogen (N)

Phosphorus (P)

Sulfur (S)

Argon (Ar)

Copper (Cu)

Gold (Au)

Silver (Ag)

Aluminum (Al)

Lead (Pb)

Zinc (Zn)

Categorize each element as a metal or nonmetal

NONMETAL

METAL

Multiple Choice

A chemical bond between a METAL and a NONMETAL is called a ___________ bond

acidic

covalent

polar

ionic

Multiple Choice

A chemical bond between one or more NONMETALs is called a ___________ bond

acidic

covalent

polar

ionic

To figure this out split the molecule by elements. Ignore the little
numbers

Example NaCl

Na is a METAL, Cl is a NON METAL
The bond between them is IONIC

Example 2: CO2 (carbon dioxide)
C is a NONMETAL, O is a NONMETAL

The bonds in this are COVALENT

Ionic or Covalent Bonds

⬤ Ions form when an atom gains or loses electrons in

its outer energy level to become stable

� Cation = The positive part. Always the metal

� Anion = The negative part. One or more nonmetals

⬤ Ionic compounds dissolve easily in water

⬤
Ionic bonds form when oppositely charged ions attract
each other

⬤
Electrolyte: Forms ions when dissolved in water

⬤
The formula of an ion always shows its charge by a “+”
or “−” after the chemical symbol

Ionic Bonds

Ionic Bonding

⬤ Covalent bonds

� Form when atoms share their outer energy to fill up

and thus become stable

� Do not ordinarily easily dissociate

in water

⬤ Hydrogen bonds

� Weak forces hold molecules in folded shapes

or in groups

� Do not form new molecules

� Found in bonds between H and F (Fluorine), H and O (oxygen) and H and N (nitrogen)

Covalent Bonds

Covalent Bonding

Why are they pretty strong?

Things H-bonds explain.

Hydrogen Bonds

How they work?
In some covalent molecules, there are partial positive and negative charges
This allows them to interact with similar molecules

Why are they pretty strong?
They form a tight network which gives it strength
In biology, A DNA molecule will have billions of these holding a double strand together

Things H-bonds explain.
The high boiling point of water compared to other similar sized molecules
How certain proteins fold

Hydrogen Bonds

Types of Bonds

Ionic: Between METALS AND NONMETALS
: Electrons are TRANSFERRED

Covalent: Between NONMETALS

: Electrons are _SHARED

Hydrogen bond: Between H and F, H and O, H and N

: A type of covalent bond

Summary of Bonds

Multiple Choice

The chemical bond between a non-metal and another non-metal will be a ________ bond.

metal

ionic

covalent

polar

Multiple Choice

Where are the nonmetals located on the periodic table?

Blue

Red

Green

Multiple Choice

Where are metals located on the periodic table?

Blue

Green

Red

Multiple Choice

What type of elements form cations?

metals

nonmetals

metalloids?

Multiple Choice

Identify the following compound as ionic or covalent: MgO

ionic

covalent

Multiple Choice

Identify the following compound as ionic or covalent: CF₄

ionic

covalent

Multiple Choice

Identify the following compound as ionic or covalent: SO₂

ionic

covalent

Multiple Choice

Identify the following compound as ionic or covalent: Ca(OH)₂

ionic

covalent

Multiple Choice

Is hydrogen considered a metal or a non-metal?

A metal

Nonmetal

Metalloid

Multiple Choice

What property of water is responsible for its high boiling point?

Covalent bonding

Ionic bonding

Hydrogen bonding

Metallic bonding

Multiple Choice

Why do HF, H2O, and NH3 have higher boiling points compared to other molecules?

They have ionic bonds.

They exhibit hydrogen bonding.

They are larger molecules.

They have covalent bonds.

Multiple Choice

Which of the following molecules exhibit unusually high boiling points due to hydrogen bonding?

CO2

NH3

Common Substances in Living

Systems

Organic Chemistry

Organic and Inorganic Chemistry

organic molecules:
Carbon-carbon or Carbon Hydrogen bonds

Size:
Larger and more complex than inorganic

Examples
Proteins, fats, nucleic acids, and carbohydrates

Inorganic Chemistry
inorganic molecules:
Water, salts, gases, acid, and bases

Size:
Smaller and simpler than organic

Examples:
Water, Carbon Dioxide, Oxygen, Hydrochloric acid, vitamins.

Categorize

Options (6)

Carbon-based molecules

Molecules tend to be large and complex

DNA, Proteins, carbohydrates, and lipids

Salts, water, gases, acids, and bases

Smaller and simpler molecules

Carbon Dioxide, Oxygen, Hydrochloric acid, and vitamins

Classify the following as either organic or inorganic chemistry

ORGANIC CHEMISTRY

INORGANIC CHEM

Water
Carbon Dioxide
Ammonia
Mineral Salts

Common inorganic molecules in

the human body

⬤ Water

� Water is essential to life

� The most abundant compound in the body, found in

and around each body cell

� Water’s slightly gluelike nature helps hold the body

together

� Water is a solvent (liquid into which solutes are

dissolved), forming aqueous solutions in the body

• Universal solvent

Inorganic Chemistry

⬤ Acids, bases, and salts

� Water molecules dissociate to form equal amounts of

H+ (hydrogen ion) and OH− (hydroxide ion)

� Acid: Substance that shifts the H+/OH− balance

in favor of H+; opposite of base

� Base: Substance that shifts the H+/OH− balance

against H+; also known as an alkaline; opposite
of acid

Inorganic Chemistry

⬤ Acids, bases, and salts

� pH: Mathematical expression of relative H+

concentration in an aqueous solution

• pH 7 is neutral (neither acid nor base)
• pH values above 7 are basic; pH values below 7 are

acidic

� Neutralization: Acids and bases mix to form salts

� Buffers: Chemical systems that absorb excess acids

or bases and thus maintain a relatively
stable pH

Inorganic Chemistry

The pH Scale

What is the pH of Blood?
What is the pH of Stomach Acid?
Is ocean water (pH= 8) acidic or basic?

Multiple Choice

What is the pH of stomach acid?

0.8

2.8

7.4

11.9

Multiple Choice

What is the pH of blood?

0.8

2.8

7.4

11.9

Multiple Choice

Acids and bases mix to form

hydrogen gas

ammonia

carbon dioxide

salt

Multiple Choice

pH above 7 is considered

neutral

acidic

basic

radioactive

Multiple Choice

pH below 7 is considered

neutral

acidic

basic

radioactive

Multiple Choice

Ocean water has a pH of 8.0. This would be considered

neutral

acidic

basic

radioactive

Multiple Choice

pH exactly 7 is considered

neutral

acidic

basic

radioactive

Multiple Choice

The most abundant compound in the body

Sodium Chloride (Salt)

Water

Carbon Dioxide

Ammonia

In humans, also known as macromolecules
The most common element in these molecules is
carbon

1. Carbohydrates also known as

sugars

2. Lipids also known as fats
3. Proteins
4. Nucleic acids

Organic Compound

⬤
Carbohydrates: Complex carbohydrates and sugars

� Contain carbon (C), hydrogen (H), and oxygen (O)

� Function of carbohydrates is to store energy

for later use

Carohydrates

Carbohydrates

Another word for Carbs is SUGARS

Two Types

1. Simple Carbs-Two Types

a. Monosaccharides
b. Disaccharides

2. Complex Carbs

Simple Sugars : Monosaccharides

●

Mono = ONE

●

Saccharide = SUGAR

●

Simple Structure:
○Consists of …
■A 5-6 carbon ring

■Hydrogens or alcohol groups
coming off the ring

� Made up of six-carbon

subunits called
monosaccharides or single
sugars (e.g., glucose)

Examples of Monosaccharides

Glucose:
a.

The preferred source of energy for the
body.

The main component in ATP
PRODUCTION

c.CELLULAR ENERGY CURRENCY_= ATP

Fructose:
a.

A Natural Sugar Found in FRUIT

Enters paths that will eventually lead to
ATP production

Galactose:
a.

Gets converted into glucose with the
body

Ribose and Deoxyribose
a.

The R in RNA and the D in
DNA

b.One of the three major components of
nucleic acids

Simple Sugars Disacharrides

●

Di = TWO

●

Sucrose = Sugars
○

●

Lactose: Sugar found in Milk
○

●

Maltose: A sugar found in malts

� Disaccharide: Double sugar

made up of two
monosaccharide units (e.g.,
sucrose, lactose)

Complex Sugars =Polysaccharides

●3 or more sugars linked

●Found in beans and whole grains

●Cellulose
○Found in plants and vegetables

●Amylose: rices and wheats

●Amylopectin: Starch found in
potatoes and corn

All of these starches break down into
smaller molecules into the body

�Polysaccharide: Complex carbohydrate
made up of many monosaccharide units
(e.g., glycogen made up of many glucose
units)

Function of Carbs

●Structurally:

○ Basis for some hormones

○MAIN FUNCTION: Breakdown into glucose

○Glucose creates ATP

○ATP (Adenosine Triphosphate) is cellular energy currency

“Good vs Bad” Carbs

●Food that are least processed and refined, like eating an orange instead of an orange cake

●Natural Carb sources, like fruits are better than processed sugars and carbs.

Cellular
Respiration:
How we get our
energy

Carbohydrates

Multiple Select

What are the two types of carbohydrates?

Complex sugars

Polyunsaturated sugars

Monounsaturated sugars

Simple sugars

Multiple Select

What are the two types of simple sugars?

Cellulose

Amylopectin

Monosaccharide

Disaccharide

Multiple Choice

Which is a monosaccharide?

lactose

sucrose

fructose

cellulose

Multiple Choice

The R in RNA is a sugar called

fructose

glucose

ribose

deoxyribose

Multiple Choice

The D in DNA is a sugar called

fructose

glucose

ribose

deoxyribose

Multiple Choice

The D in DNA is a sugar called

fructose

glucose

ribose

deoxyribose

Multiple Choice

The D in DNA is a sugar called

fructose

glucose

ribose

deoxyribose

Multiple Choice

The monosaccharide found in fruit is called

glucose

sucrose

lactose

fructose

Multiple Choice

Another name for table sugar is

glucose

lactose

sucrose

fructose

Multiple Choice

The disaccharide found in milk is called

glucose

lactose

sucrose

fructose

Multiple Choice

The complex sugar found in plant cell walls is called

glucose

cellulose

starch

sucrose

⬤ Lipids: Fats and oils

� Triglycerides

• Made up of one glycerol unit and three fatty acids
• Store energy for later use

� Phospholipids

• Similar to triglyceride structure, except with only two

fatty acids, and with a phosphorus-containing group
attached to glycerol

• The head attracts water (hydrophilic) and the double tail

does not (hydrophobic), thus forming stable double
layers (bilayers) in water

• Form membranes of cells

Organic Chemistry

Triglyceride

Phospholipids

⬤ Lipids: Fats and oils

� Cholesterol

• Molecules have a steroid structure made up of multiple

rings

• Cholesterol stabilizes the phospholipid tails in cellular

membranes

• Cholesterol is converted into steroid hormones by the

body

Organic Chemistry

Cholesterol

Multiple Choice

Lipids that are a liquid at room temp are called

waxes

fats

butters

oils

Multiple Choice

Triglycerides are made of

three fatty acids and one glycerol molecule

three fatty acids and two glycerol molecules

four fatty acids and one glycerol molecule

two fatty acids and one glycerol molecule

Multiple Choice

The structure of a phospholipid contains

A single hydrophobic tail and a hydrophilic tail.

A hydrophilic head and two hydrophobic tails.

Two hydrophilic heads and one hydrophobic tail.

A hydrophobic head and two hydrophilic tails.

Fill in the Blanks

100

Match

Match the following function with the type of lipid

Converted into hormones like steroid

Used for energy storage

Forms the cell membrane

cholesterol

triglycerides

phospholipids

101

⬤ Proteins

� Very large molecules made up of amino acids held

together in long, folded chains by peptide bonds

� Structural proteins

• Form various structures of the body
• Collagen: Fibrous protein that holds many tissues

together

• Keratin: Forms tough, waterproof fibers in the outer

layer of the skin

Organic Chemistry

102

Protein

103

⬤ Proteins

� Functional proteins

• Participate in chemical processes of the body
• Examples: Hormones, cell membrane channels

and receptors, enzymes

• Enzymes

� Catalysts: Help chemical reactions occur

� Lock-and-key model: Each enzyme fits a particular

molecule like a key fits into a lock

Organic Chemistry

104

Enzyme Action

105

Multiple Choice

Fibrous proteins that holds many tissues together

Collagen

Elastin

Keratin

Actin

106

Multiple Choice

Structural protein that forms the tough, waterproof outer layer of the skin

keratin

collagen

elastin

hyaluronic acid

107

Multiple Choice

Enzymes are ________ that act as ________.

proteins, catalysts

amino acids, proteins

proteins, amino acids

catalysts, carbohydrates

108

Multiple Choice

The ____________________ mechanism describes how each substrate must fit into the enzyme.

lock and key

hammer and nail

jigsaw puzzle

seesaw

109

⬤
Nucleic acids

� Made up of nucleotide units

• Sugar (ribose or deoxyribose)
• Phosphate
• Nitrogen base (adenine, thymine or uracil, guanine, cytosine)

� Deoxyribonucleic acid (DNA)

• Used as the cell’s “master code” for assembling proteins
• Uses deoxyribose as the sugar and uses A, T (not U), C, and

G as bases

• Forms a double helix shape

Organic Chemistry

110

Multiple Choice

What are the three main parts of a nucleic acid?

Carbohydrates, proteins, lipids

Amino acids, fatty acids, glycerol

Phosphate group, sugar, nitrogenous base

Enzymes, coenzymes, substrates

111

Multiple Choice

What are the 4 bases for a DNA?

Guanine, Thymine, Cytosine, Adenine

Adenine, Thymine, Cytosine, Uracil

Adenine, Uracil, Cytosine, Guanine

Adenine, Thymine, Cytosine, Guanine

112

Deoxyribonucleic Acid

113

⬤
Nucleic acids

� Ribonucleic acid (RNA)

• Used as a temporary “working copy” of a gene (portion of the

DNA code)

• Uses ribose as the sugar and uses A, U (not T), C, and G as

bases

� By directing the formation of structural and functional

proteins, nucleic acids ultimately direct overall body
structure and function

� Adenosine triphosphate (ATP): A modified nucleotide used

to transfer energy from nutrients to cellular processes, thus
acting as an energy-transfer “battery”

Organic Chemistry

114

Categorize

Options (8)

single stranded

Adenine, Guanine, Cytosine, and uracil

Ribose

Intermediate in protein synthesis

Contains the blueprint for protein synthesis

Adenine, Guanine, Cytosine, Thymine

Double stranded helix

depxyribose

What are the differences between DNA and RNA?

RNA

DNA

115

Adenosine Triphosphate

Chapter 2

Chemistry of Life

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