Biology Chemistry Terms: Radioactive Decay & Bonds Study Set

List the levels of organization (smallest to largest)

subatomic particles, atoms, functional groups, simple molecules, macromolecules, membrane, compartment/organelle, cell, tissue, organ, organ system, organism

organism

entire living entity can be multicellular or single-celled

organ system

two or more organs working together for some function

examples of organims

plants, animals, bacteria

example of an organ system

cardiovascular system

organ

2 or more tissue types together for structure

examples of organs in the cardiovascular system

heart (cardio), blood vessels (vascular)

tissue

group of similar cells joined together

examples of tissues in the cardiovascular system

cardiac muscle and epithelial tissue

cell ****

smallest living unit

compartment/organelle

in eukaryotic cells, they are membrane-enclosed domains

membrane example

phospholipid bilayer

macromolecules example

DNA, polysaccharides

simple molecules example

water, carbon dioxide, methane

functional groups

atom or group of atoms that have particular properties

what do functional groups do?

confer their properties to molecules that contain them

atoms

smallest units of elements

subatomic particles

protons, neutrons, electrons

What do protons determine?

the identity of an element

what do electrons determine?

chemical reactivity

what are the biologically important molecules?

organic, inorganic, essential chemical elements and heavy metals

organic molecules

molecules that contain carbon (minimum requirement) and usually has carbon bonded to hydrogen

examples of organic molecules

carbohydrates, fats, proteins

inorganic molecules

most do not contain carbon

essential chemical elements

-112 total elements

-92 Naturally occurring

-20-25 are essential elements.

CHNOPS

Carbon, Hydrogen, Nitrogen, Oxygen, Phosphorus, Sulfur

what does chnops make up?

about 98% of human body

examples of trace elements

cobalt, copper, manganese, selenium

heavy metals

important but not essential

examples of heavy metals

arsenic, cadmium, mercury, lead

families of biologically important molecules

carbohydrates, lipids/fats, amino acids/proteins, nucleic acids (dna/rna)

what do families of biologically important molecules have?

they recognizable functional groups

Examples of functional groups

hydroxyl, methyl, phosphate

hydroxyl group

-OH

methyl group

-CH3

phosphate group

-PO4

atoms are....

the building blocks of matter, made of subatomic particles

Electrons charge

negative 1

protons charge

positive 1

neutrons charge

neutral (no charge)

Where are electrons located?

outside the nucleus

Where are protons and neutrons located?

inside the nucleus

atomic number

number of protons, identifies what element the atom is

atomic mass/mass number

number of protons + number of electrons + number of neutrons

how do all atoms start?

electrically neutral

what are elements?

unique substances that make up matter

what is each element composed of?

1 kind of atom

isotope

element having a different number of neutrons (same number of protons)

radioactive decay

1. low energy emitters 2. high-energy emitters 3. regulation +safety

What is radioactive decay in the isotope of hydrogen; tritium

When a neutron is added to proton along with energy, it forms Beta rays which is very unstable

example of low-energy emitters

medical imaging

example of high-energy emitters

damaging to cells, chemotherapy *damaging

what are ions

charged atoms or groups of atom

types of ions

cations and anions

cations

positively charged ions

anions

negatively charged ions

examples of ions

ionization of sodium and chlorine

molecules

2 or more atoms held together by chemical bonds

what happens if atoms are different in a molecule what is it called?

a compound

mixtures

2 or more components physically intermixed, but NOT chemically bonded

types of mixtures

solution and suspension

what is a solution

solute plus solvent

solute

that which is dissolved

ex. minerals

solvent

that which does the dissolving

ex. water

suspension

large particles that are not homogenously mixed and scatter light

what is the universal solvent?

water because it is a aqueous solution/environment

types of chemical bonds

ionic bonds, covalent bonds, hydrogen bonds, van der waals forces/london dispersion forces

ionic bond

bond between oppositely charged atoms/groups

what is the bond energy of an ionic bond

3-7 kcal/mol, weak, and in aqueous environments

example of an ionic bond

NaCl, separates readily in water

covalent bond

atoms share valence electrons, the electrons in the outermost energy level, can be single, double, or triple

bond energy of covalent bond

50-110 kcal/mol STRONG

octet rule definition #1

atoms like to have 8 electrons in the outermost energy level

octet rule definition #2

atoms like to have filled outermost energy levels MOST STABLE

what does a not full outermost level cause

increased reactivity

what else can covalent bonding form

compounds

electronegativity

pull on shared electrons in a covalent bond

nonpolar covalent bond

electrons are shared equally between 2 electrons

polar covalent bond

electrons are shared unequally

example of nonpolar covalent bond

C-C and C-H

example of polar covalent bond

O-H

examples of electronegativity

ionization of Na and Cl and water molecules

hydrogen bond

sharing of hydrogen between and oxygen or nitrogen of one molecule with the oxygen or nitrogen of another molecule

bond energy of hydrogen bonds

3-7 kcal/mol, weak

hydrogen bonds are what two kinds

intramolecular or intermolecular

intermolecular

between molecules

intramolecular

within the same molecule

what properties do hydrogen bonds give to water

special properties: cohesiveness, surface tension, ability to dissolve solutes

why is hydrogen bonding important for the body?

allows proper folding and structure of proteins and dna

where does surface tension occur

At all air-water interfaces

hydrogen bonds: surface tension in water molecules

Hydrogen bonds at interface are stronger than in bulk solution/water, causing it to be strong enough to withstand force

van der waals forces/london forces

brief, weak electron interactions between nonpolar molecules

what is the bond energy of van der waals forces/ london forces

1 kcal/mol, very weal

When are van der Waals forces strongest?

accumulation of forces

chemical interactions: hydrophilic-hydrophobic interactions

hydrophilic loves hydrophilic and hydrophobic loves hydrophobic

how is a substance hydrophilic?

if it has charges

if a substance does not have a charge how can it be hydrophilic?

if it offers hydrogen bonding opportunities

Characteristics of hydrophobic reactions

the arrangement in energetically unfavorable; hydrophobic molecules are excluded from hydrophilic interactions

Does sodium chloride dissolve in water?

Yes

The sodium and chlorine ions are separated as water gets in between them.

How does the charge shielding effect impact sodium chlorine being dissolved in water?

The positively charged hydrogens of a water molecule surround the negatively charged chlorine ion and the negatively charged oxygens of a water molecule surround the positively charged sodium ion.