Biochemistry (Atoms And Molecules Part 1)

Front 1

1 What is the unit of an element?
2 What is Atomic Number?
3 What is Atomic Mass?

Back 1

1 An Atom
2. Number of Protons
3. Weight, Neutrons + Protons

Front 2

1 What is an Isotope
2 How can they be used?

Back 2

1 The same element, but with a different number of neutrons.

2. Tracking of movement of materials in the body
. Treatment of Cancer Cells

Front 3

Molecules

Back 3

-A molecule is the bonding together of two or more atoms

-Most elements form molecules

-Atoms form molecules in an effect to fulfill their outer electron shell

-The closest valence ring(to the nucleus) holds two electrons, and all other valence shells hold 8

Front 4

Noble Gases

Back 4

-Their electron shells are filled

Front 5

Chemical Bonds
(Covalent)

Back 5

-Share their valence shell with another atom
-Very strong bond(Takes a lot of energy to break
-Denoted as a stick
-Comes in Single, Double, or Triple, such in the case of nitrogen
-The number of covalent bonds an atom can form is equal to the number of additional electrons needed to fill its out shell.

Front 6

Methane

Back 6

Is the smallest organic molecule

Front 7

(Polar Covalent Bonds)

Back 7

-Are covalent bonds where the electrons are not shared equally

-This occurs when one atom in the molecule has a higher electronegativity which is when one nucleus(in the compound) may exert a greater attractive for on the electron pair so the pair tends to be closer to that atom.

-Results in one side of the molecule(atom that has higher electronegativity) to be slightly negative, while the other side (atom or atoms) to be slightly positive

Front 8

Ion

Back 8

Ions are electrically charged particles.

-Occurs when electronegativity in one atom is MUCH higher, enough to rip away an electron

-The atom that contains a positive charge, the cation is also termed the donor

-The atom that contains a negative charge, or anion also called the receiver

Front 9

What is a molecule?
How does it differ from an ion?

Back 9

-A molecule is an electrically neutral group of at least two atoms held together by covalent chemical bonds.


-Molecules are distinguished from ions by their electrical charge.

Front 10

Electronegitivity

Back 10

The unequal sharing of a pair or pairs of electrons between atoms

-A very high electronegativity will result in ion formation

-A slight electronegitivity will result in polar covalent bond formation

Front 11

Methane

Back 11

Is the smallest organic molecule

Front 12

(Polar Covalent Bonds)

Back 12

-Are covalent bonds where the electrons are not shared equally

-This occurs when one atom in the molecule has a higher electronegativity which is when one nucleus(in the compound) may exert a greater attractive for on the electron pair so the pair tends to be closer to that atom.

-Results in one side of the molecule(atom that has higher electronegativity) to be slightly negative, while the other side (atom or atoms) to be slightly positive

Front 13

Ion

Back 13

Ions are electrically charged particles.

-Occurs when electronegativity in one atom is MUCH higher, enough to rip away an electron

-The atom that contains a positive charge, the cation is also termed the donor

-The atom that contains a negative charge, or anion also called the receiver

-Some elements can gain multiple charges by gaining or losing more than one electron

Front 14

What is a molecule?
How does it differ from an ion?

Back 14

-A molecule is an electrically neutral group of at least two atoms held together by covalent chemical bonds.


-Molecules are distinguished from ions by their electrical charge.

Front 15

Electronegitivity

Back 15

The unequal sharing of a pair or pairs of electrons between atoms

-A very high electronegativity will result in ion formation

-A slight electronegitivity will result in polar covalent bond formation

Front 16

What is an ionic Bonds?
What is a salt?

Back 16

-Bonds formed as the result of the electrical attraction between ions bearing opposite charges

-Ions that can form stable solid compounds are referred to as salts.

Front 17

Hydrogen Bonds

Back 17

A hydrogen bond is the attractive interaction of a hydrogen atom with an electronegative atom.

-The hydrogen must be covalently bonded to another electronegative atom to create the bond

-May occur between molecules, (intermolecularly) or within different parts of a molecule (intra-molecularly)

-They are responsible for maintaining the 3d shape of DNA and Protein

-Not restricted to water

Front 18

Hydrophilic

Back 18

Any molecule that is polar may interact with another molecule that is a polar through the week attractions of hydrogen bonds.

-If a polar molecule acts with water in this way, then it is referred to as hydrophilic ( water lover)

Front 19

Hydraphobic

Back 19

-Nonpolar molecules tend to react with other non polar molecules.

EXAMPLE :
-Carbon forms non polar bonds with hydrogen, and molecules containing only carbon and hydrogen referred to as hydrocarbons; are non polar, in water these molecules tend to aggregate with eachother rather than the water (h2o, polar)

Front 20

Water

Back 20

-Universal solvent of life
-A polar molecule that may form hydrogen bonds
-High specific heat
-It becomes less dense when freezes

Front 21

Cohesion

Back 21

-In liquid water, water molecules are able to move about continuously forming and reforming hydrogen bonds

-These hydrogen bonds explain the cohessive strength of liquid water.

-This cohession is defined as water molecules sticking to other water molecules, or the capacity of water molecules to come apart when under pressure

Front 22

Surface Tension

Back 22

The surface of liquid water when exposed to air is hard to puncture because the water molecules on the surface are hydrogen bonded to the water molecules below them

Front 23

Acids

Back 23

-When some substances dissolve in water, they release H+, (hydrogen ions) which are actually positively charged protons

-Acids that fully ionize in solution are called strong acids

-Acid that partially ionize in solution are strong acids

< 7pH

Front 24

Bases

Back 24

-When some substances disolve in water, they accept H+
-Some bases do this by releasing OH- which combines with H+ to form h2o

> pH 7

Front 25

The connection between hydrogen bonds and polar molecules

Back 25

The polarity of water molecules permits hydrogen bonding

Front 26

Buffers

Back 26

Substances that prevent harmful changes in pH by accepting H+ when that ion is in excess and donating H+ when it is depleted

-Helps with homeostasis (blood chemistry)

Front 27

Dehydration Synthesis(Endergonic) (Anabolism)

Back 27

A chemical reaction that removes a molecule of water when monomer sub units are being added to make a longer polymer chain.

-The existing polymer has either an H, or OH that forms with the end of the new monomer(subunit)'s H or OH to form a water molecule, they replace the lost bond with a bond to each other

Front 28

Hydrolysis(Exergonic)(Catabolism)

Back 28

A catabolic process in which an existing polymer is split into monomer subunits.

Front 29

Catabolism

Back 29

The set of metabolic pathways that break down molecules

Front 30

Anabolism

Back 30

The set of metabolic pathways the make molecules.