Chemistry and Biochemistry

Adp

(Adenosine Diphosphate) The compound that remains when a phosphate group is removed from ATP, releasing energy

Formula for monosaccharides

(CH2O)n, n is the number of carbons in the sugar.

methylene chloride

(Dichloromethane) skin, eye, and mucous membrane irritation, depresses the CNS, COHb-emia, angina pectoris, A3

The formula for a compound containing ammonium ion(s) and phosphate ion(s) is _______

(NH4)3PO4

Atp

(adenosine triphosphate) main energy source that cells use for most of their work

Solve the following equation forx:5x- 3 = 3x- 5

-1

Solve the following equation forx: -4x+ 2 = 22

-5

Which of the following quantities is equivalent to 594 mg?

0.594 g

Differences between mixtures and compounds

1. No chemical bonding between components of a mixture. 2. Mixtures can be separated by straining, filtering, evaporation while compounds can only be separated by chemical means. 3. all compounds are homogenous while mixtures are either homogenous or heterogenous.

Why do the electrons farthest from the nucleus have the greatest potential energy?

1. it takes more energy to overcome the nuclear attraction and reach the more distant energy levels. 2. Are more likely to interact chemically with other atoms.

How many protons and electrons are there in the magnesium (Mg2+) ion?

12 protons and 12 electrons

Which of the following numbers is notexpressed in proper scientific notation? a)5.6× 10-3 b)12.6× 102 c)4× 108 d)6.02× 1023

12.6 × 10^2

carbon in body

18.5% A primary component of all organic molecules which includes carbohydrates, lipids, proteins, and nuclei acids

What is the charge on the Fe ion in the ionic compound with the formula, Fe2O3?

3 plus

Nitrogen in body

3.2% A component of proteins and. nuclei acids

The value 3.0 × 10^8is equal to ______.

300 000 000

A bag contains 100 jellybeans. If 32 of them are red, what percent of the jellybeans in the bag are red?

32%

According to the graph, what temperature was the tea after 60 min?

35 C

Pentose

5 carbon sugar (ribose, deoxyribose)

A bouquet of flowers has 4 red roses, 6 pink carnations, and 10 white daisies in it. What percent of the flowers in the bouquet are daisies?

50%

Hexose

6 carbon sugar, blood sugar

If there are 25 marbles in a box and 9 of them are blue, what percent of the marbles are notblue?

64%

Oxygen in body

65% A major compound of both organic and inorganic molecules, used in the production of cellular energy

What number occupies the hundredths place in 547.982?

8

hydrogen in body

9.5% A component of all organic molecules, as a ion, it influences the pH of body fluids.

anabolic activities

A + B --> AB, buildup of larger molecules from smaller ones, ex. steroids build muscle, amino acids combine to make protein molecules

physical change

A change in a substance that does not involve a change in the identity of the substance

chemical change

A change in matter that produces one or more new substances

polyatomic ion

A charged group of covalently bonded atoms

covalent bond

A chemical bond that involves sharing a pair of electrons between atoms in a molecule. Example, hydrogen with a single valence electron can bond with another hydrogen to make molecules of hydrogen gas that satisfies stability. While, also hydrogen can also bond with other elements to make compounds (carbon) that satisfy valence stability, example methane gas, CH4

molecular formula

A chemical formula that shows the number and kinds of atoms in a molecule, but not the arrangement of the atoms.

synthesis (combination) reaction

A chemical reaction in which larger, more complex atoms or molecules are formed from simpler ones.

dehydration reaction

A chemical reaction in which molecules combine by removing water

dehydration synthesis

A chemical reaction in which two molecules covalently bond to each other with the removal of a water molecule.

redox reaction

A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation-reduction reaction. Ex. formation of NaCl, sodium is oxidized when it loses an electron and chlorine is reduced when it gains an electron.

hydrolysis reaction

A chemical reaction that breaks apart a larger molecule by adding a molecule of water

Mixtures

A combination of two or more substances that are not chemically combined

Which one of the following is an example of a compound?

A compound has two or more elements chemically bound together and cannot be separated by physical means.

Disaccharide

A double sugar, consisting of two monosaccharides joined by dehydration synthesis.

molecule

A group of atoms bonded together

Prostaglandins

A group of bioactive, hormone-like chemicals derived from fatty acids that have a wide variety of biological effects including roles in inflammation, platelet aggregation, vascular smooth muscle dilation and constriction, cell growth, protection of from acid in the stomach, and many more.

triacylglycerol

A lipid consisting of three fatty acids linked to one glycerol molecule; also called a fat or triglyceride.

Cholesterol

A lipid that forms an essential component of animal cell membranes and acts as a precursor molecule for the synthesis of other biologically important steroids.

Electronegativity

A measure of the ability of an atom in a chemical compound to attract electrons. Examples, oxygen, nitrogen, chlorine.

Cobalt-60 radiation

A method of institutional bulk sterilization used by manufacturers to sterilize prepackaged equipment using ionizing radiation. Used to destroy localized cancers

Colloid

A mixture containing small, undissolved particles that do not settle out. Heterogenous mixtures

Suspension

A mixture in which particles can be seen and easily separated by settling or filtration. Heterogenous mixtures

Solutions

A mixture where substances are distributed evenly. Has a solvent & solute.

difference between compound and molecule

A molecule is formed when two or more atoms join together chemically. A compound is a molecule that contains at least two different elements. All compounds are molecules but not all molecules are compounds.

endergonic reaction

A non-spontaneous chemical reaction in which free energy is absorbed from the surroundings. Ex. anabolic reactions

Polypeptide

A polymer (chain) of many amino acids linked together by peptide bonds.

molecular chaperones

A protein that helps other proteins fold or refold from a partially denatured state.

percent

A ratio that compares a number to 100

electron acceptor

A reactant that gains an electron and is reduced in a reduction-oxidation reaction.

electron donor

A reactant that loses an electron and is oxidized in a reduction-oxidation reaction.

chemical equation

A representation of a chemical reaction that uses symbols to show the relationship between the reactants and the products

pure substance

A sample of matter, either a single element or a single compound, that has definite chemical and physical properties

ammonia

A small, very toxic molecule (NH3) produced by nitrogen fixation or as a metabolic waste product of protein and nucleic acid metabolism.

Substrate

A specific reactant acted upon by an enzyme

alpha helix

A spiral shape constituting one form of the secondary structure of proteins, arising from a specific hydrogen-bonding structure.

exergonic reaction

A spontaneous chemical reaction in which there is a net release of free energy. Ex catabolic and oxidative reactions

Reactants

A starting material in a chemical reaction

starch

A storage polysaccharide in plants consisting entirely of glucose.

compound

A substance made up of atoms of two or more different elements joined by chemical bonds

proton donor

A substance that releases hydrogen ions in detectable amounts; an acid.

proton acceptor

A substance that takes up hydrogen ions in detectable amounts. Commonly referred to as a base. Ex. hydroxides, magnesium hydroxide, sodium hydroxide

Glycerol

A three-carbon alcohol to which fatty acids are covalently bonded to make fats and oils. Modified simple sugar. Glycerol backbone is the same in all neutral fats except the fatty acid chains vary

methane gas

A type of greenhouse gas that is produced in agriculture practices such as raising cattle and farming rice. CH4

ribonucleic acid (RNA)

A type of nucleic acid consisting of nucleotide monomers with a ribose sugar and the nitrogenous bases adenine (A), cytosine (C), guanine (G), and uracil (U); usually single-stranded; functions in protein synthesis and as the genome of some viruses.

Macromolecules

A very large organic molecule composed of many smaller molecules

Italian dressing contains olive oil and vinegar, which will separate out from each other if left to sit. This makes the dressing a:

A) Heterogeneous mixture

A homogeneous mixture is also called a ____________. A) solution B) pure substance C) heterogeneous mixture D) liquid

A) solution A solution is a type of homogeneous mixture composed of two or more substances.

catabolic activities

AB --> A + B, breakdown of larger molecules into smaller molecules, Example, bonds of large glycogen are broken to release simpler molecules of glucose sugar

Cytosol (Cytoplasm)

ALL CELLS HAVE THIS! It's the fluid inside of every living cell where organelles float. colloid

Aspartic Acid

Acidic, Asp, D

How many significant figures does the answer of 2.5 + 9.520 contain?

Adding the numbers together gives 9.520 + 2.5 = 12.020. Decimal place determines the sig figs for addition and subtraction, and the given value 9.5 tells us our answer will have one decimal place. Rounding down to 12.0 is our final answer to three significant figures.

Metallochaperones

Aid the transit of certain metal jobs across the plasma membrane helping to avoid excesses which might be toxic

Predict the chemical formula for the ionic compound formed by Al³⁺ and C₂H₃O₂⁻

Al(C₂H₃O₂⁻)3 aluminum acetate

Predict the chemical formula for the ionic compound formed by NH₄⁺ and PO₄³⁻

Ammonium Phosphate, highly unstable, (NH4)3PO4

noble gas notation

An abbreviated electron configuration of an element in which filled inner shells are represented by the symbol of the preceding noble gas in brackets

silver nitrate

An antiseptic and astringent with caustic properties, AgNO3

Aufbau Principle

An electron occupies the lowest-energy orbital that can receive it

electron shell

An energy level representing the distance of an electron from the nucleus of an atom.

Glycogen

An extensively branched glucose storage polysaccharide found in the liver and muscle of animals; the animal equivalent of starch.

ammonium phosphate

An extinguishing agent used in dry chemical fire extinguishers that can be used on Class A, B, and C fires.

radiation sickness

An illness that results from excessive exposure to nuclear radiation

Hydroxyl ion (OH-)

An ion liberated when a hydroxide (a common inorganic base) is dissolved in water.

salt

An ionic compound made from the neutralization of an acid with a base. Ex. calcium carbonate, potassium chloride, calcium phosphates

Electrolyte

An ionic compound whose aqueous solution conducts an electric current

Isotopes

Atoms of the same element that have different numbers of neutrons, or isotopes of the same element has the same number of protons and electrons but differ in neutrons.

Predict the chemical formula for the ionic compound formed by Au³⁺ and HSO₃⁻

Au3plus + 3HSO3 -> Au(HSO3)3

Lysine

Basic 3 carbon chain plus one methylene to amino, it lies ("Lys") about the 3 carbon trend

Assume imaginary compound XY has a polar covalent bond. How does its charge distribution differ from that of XX molecules?

Because X and Y are different atoms, one is bound to be more electronegative than the other. There will be a separation of charge in XY. which is a dipole. In XX, the atoms are the same in equal e sharing, no dipole forms.

Which of the following combinations would form a solution? I) Water and ethanol II) Sand and table salt III) Oxygen and nitrogen IV) Oil and vinegar

Because water and ethanol are both polar liquids, one dissolves in the other to form a liquid-liquid solution. The air around us has a uniform composition at a given altitude, and is made up of a gaseous homogeneous mixture (solution) of primarily oxygen and nitrogen.

Sodium bicarbonate

Both ionic and covalent compound

hydrolysis

Breaking down complex molecules by the chemical addition of water

Some liquid in a jar can be separated by physical means into two separate liquids, which can then be separated no further. The liquid is a(n): A) Compound B) Element C) Mixture D) Pure substance

C. Mixture If a sample of matter (the liquid in the jar) can be separated by physical means, it's a mixture. Otherwise, it's a pure substance that can either be an element or compound.

table sugar

C12H22O11-Compound

Formula for glucose

C6H12O6

cellular respiration equation

C6H12O6+6O2--->6CO2+6H2O+ATP energy

glucose molecular weight

C6H12O6, C=6x12.011, H=12x1.008, O=6x15.999, Added together Is 180.156

organic acid group

COOH releases H+ ions

Predict the chemical formula for the ionic compound formed by Ca²⁺ and ClO₃⁻

Ca(ClO3)2 calcium chlorate

Predict the chemical formula for the ionic compound formed by the elements Ca and Br

CaBr2

Polysaccharides

Carbohydrates that are made up of more than two monosaccharides

Enzymes

Catalysts for chemical reactions in living things

stress proteins

Cells synthesize "stress proteins" when homeostasis is disrupted

induced fit model

Change in the shape of an enzyme's active site that enhances the fit between the active site and its substrate(s)

Denatured

Change the shape of an enzyme so that it can no longer speed up a reaction.

Which of the following forms of energy are in use during vision? (a) chemical,(b)electrical,(e)mechanical,

Chemical

Catalysts

Chemical agents that selectively speed up chemical reactions without being consumed by the reaction.

intramolecular bonds

Chemical bonds between atoms in a molecule; ionic, covalent, or metallic bonds

Calcium chlorate/ CaClO3

Chlorinated lime, chloride of lime, calcium salt of chloric acid, strong oxidizer, used as a herbicide and pyrotechnics

which of the following compounds does not exhibit covalent bonding

CoCl2

Collagen

Composite of the helical tropocollagen molecules packed together side by side to form a rope like structure

Water (H2O)

Compound broken down during the light reactions of photosynthesis. Provides electrons & protons (hydrogen ions) for later use, This is a dipole or a polar compound where the electrons of hydrogen are slightly positive and oxygen is very electronegative, and electrons are generally negative charged, it is causes this compound to be polar covalent bond or dipole.

organic compounds

Compounds that contain carbon, covalently bonded molecules

OF2, CuO, SeO2

Covalent, ionic, Covalent

Predict the chemical formula for the ionic compound formed by the elements Ca and Br

Cs3P

The subatomic particles responsible for the chemical behavior of atoms are(a) electrons,(b)ions,(c)neutrons （d)protons

Electrons

Activation energy

Energy needed to get a reaction started

lipids

Energy-rich organic compounds, such as fats, oils, and waxes, that are made of carbon, hydrogen, and oxygen. Insoluble but dissolve readily in other lipids and organic solvents

John Dalton

English chemist and physicist who formulated atomic theory and the law of partial pressures

Which scientist developed the nuclear model of the atom?

Ernest Rutherford

The Rapid Antigen Test in the previous example is a(n) _____.

Experiment

fat synthesis

Fats are composed of a glycerol molecule bonded to three fatty acids. Fats provide for long term energy storage. They also insulate the body and pad vital organs, and they provide the materials to build many fat-based hormones. Fats are high energy molecules as seen by all of the hydrogen atoms bonded to the carbons on the fatty acid tails. Fats must be broken down into the glycerol and the three individual fatty acid tails before they can be absorbed from the small intestine into the blood.

A deficiency in this element can be expected to reduce the hemoglobin content of blood:(a)Fe,(b)I,(c)F,(d)Ca,

Fe iron

Predict the chemical formula for the ionic compound formed by Fe³⁺ and O²⁻

Fe2O3

Iron (111) oxide

Fe2O3, inorganic compound, one of the main oxides of iron, rust, hydrated ferric oxide

Which of the following states of matter are considered fluids? I) Solid II) Liquid III) Gas

Fluids flow under pressure. This is a property of both liquids and gases.

gamma emission

Form of radioactive decay that occurs when an unstable nucleus emits extremely high frequency electromagnetic radiation, greatest penetrating power towards tissue

ionic bond

Formed when one or more electrons are transferred from one atom to another

Which of the following are controlled variables in an experiment on the effects of a new high blood pressure medication on men with a family history of heart disease?

Gender and genetic predisposition

strong acids

HCl, HBr, HI, HNO3, H2SO4, HClO4

Predict the chemical formula for the ionic compound formed by Hg₂²⁺ and CO₃²⁻

Hg2CO3, mercury carbonate

Water properties

High heat capacity; polar; molecules of water cling together; a great solvent; liquid at room temp; frozen water is less dense then liquid water, high heat of vaporization, reactivity, cushioning

Grape juice is an example of a(n)

Homogeneous mixture If a sample of matter is a mixture that is uniform in composition throughout, it's a homogeneous mixture.

Doctors employ the Scientific Method to diagnose patients. A patient visits a doctor's office and presents the following symptoms: fever, sore throat, and headache. The doctor looks intothe patient's throat and notes that the tonsils are inflamed. The doctor suspects that the patient has strep. She then swabs the throat to perform a Rapid Antigen Test. The physician's suspicion is an example of a(n) _____.

Hypothesis

Because electron energy levels are quantized, which of the following is true? I) Atomic emission spectra are a series of discrete lines. II) Atomic emission spectra are continuous. III) Electrons may only occupy a discrete set of energy levels. IV) Electrons may occupy a continuous range of energy levels.

I and III

coenzyme

If the cofactor is an organic molecule.

Which one of the following is NOT an example of a physical change?

In a chemical change, one substance must be converted into another. In electrolysis, the chemical bonds in water are broken to release elemental hydrogen and oxygen as gases.

chemical equilibrium

In a chemical reaction, the state in which the rate of the forward reaction equals the rate of the reverse reaction, so that the relative concentrations of the reactants and products do not change with time.

KNO3

Ionic and covalent bonds

ZnS

Ionic compound

salts

Ionic compounds that can be formed by replacing one or more of the hydrogen ions of an acid with another positive ion

KCL, CrCl3, Cl2O

Ionic, ionic, convalent

BaO, Fe2O3, ZnO

Ionic, ionic, ionic

Temperature

Kelvin (K)

strong bases

LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2 dissociate in water easily and quickly tie up hydrogen plus.

The formula magnesium oxide is____

MgO

Nitrogen gas

N2, is the atmosphere's most abundant element making up 78% of the volume in the troposphere. It is also a triple bond between two of the same element.

sodium chloride

NaCl table salt, sodium with atomic number 11, has only 1 valence shell electron, goes through cation by losing that 1 valence shell in its third energy level and becomes stable. Chlorine with atomic number 17, needs a valence electron and goes through anion to become stable. Ionic bond

baking soda

NaHCO3-compound

neutral fats

Neutral fats are non polar, uncharged triglycerides that have no acidic or basic groups. Large molecules consisting of hundreds of atoms.

Which one of the following is an example of an element?

Nickel

Cofactor

Non-protein helpers that may be bound tightly to the enzyme as a permanent resident, or may bind loosely and reversibly along with the substrate.

Oxygen gas

O2, colorless and odorless. It will make a flame burn brighter and faster, capable of making a burning ember turn back into a flame, and it is required for combustion. It is also a double bond between two of the same element

ozone gas

O3-Element

beta pleated sheet

One form of the secondary structure of proteins in which the polypeptide chain folds back and forth, or where two regions of the chain lie parallel to each other and are held together by hydrogen bonds.

radium 226

One of the first radioactive elements associated with biological damage. Used to destroy localized cancers

Three students measure the volume of a liquid using a graduated cylinder. In a separate experiment, the actual value volume of the liquid is 152 mL. Which set of data is the most precise?

Precision is when all outcomes are in the range of uncertainty of one another and accuracy is when the average outcome is in the range of uncertainty of where it should be. Precision and accuracy are independent of one another. An outcome can be precise but not accurate, accurate but not precise, accurate and precise, or neither accurate nor precise. For Student 2, the data have least amount of uncertainty between measurements, the data are precise even though they are not particularly accurate.

heat-shock proteins

Proteins that help maintain integrity of other proteins that would normally be denatured in extreme heat.

The symbol for the ion formed by sulfur is ______.

S2-

All af the following are examples of the four major elements contributing to body mass except(a)hydrogen, (b) carbon,(c)nitrogen,(d)sodium,

Sodium

Gasoline is composed of a variety of different liquid hydrocarbons, which do not separate as time passes. Gasoline is an example of a:

Solution- Gasoline is a homogeneous liquid-liquid mixture of a variety of different hydrocarbons, and other soluble additives. Therefore, it is a solution.

Predict the chemical formula for the ionic compound formed by Sr and Cl

SrCl2

weak bases

Substances capable of accepting hydrogen but do not completely ionize in solution ex. baking soda

The mass number of an atom is(a)equal to the and neutrans,(c) the sum of all of its subatomic particles （d)the average of the mass numbers of all of its isotopes.

Sum of protons and neutrons

Factors that influence the rate of chemical reactions

Temperature, particle size, concentration, and catalysts

What if the atom has more than 8 electrons beyond shell 2?

The atom can contain more than 8 electrons, but only 8 electrons are allowed to participate in bonding.

Guanine

The base that pairs with Cytosine in DNA

Adenine

The base that pairs with Thymine in DNA

Alkalosis

The buildup of excess base (lack of acids) in the body fluids, ph above 7.5

peptide bond

The chemical bond that forms between the carboxyl group of one amino acid and the amino group of another amino acid

products

The elements or compounds produced by a chemical reaction.

primary structure

The first level of protein structure; the specific sequence of amino acids making up a polypeptide chain.

double helix

The form of native DNA, referring to its two adjacent polynucleotide strands wound into a spiral shape.

quaternary structure

The fourth level of protein structure; the shape resulting from the association of two or more polypeptide subunits.

valence shell

The outermost energy shell of an atom, containing the valence electrons involved in the chemical reactions of that atom.

The picture is best described as a liquid mixture. Liquids do not have a definite shape but do not fill the entire container, so the particles are found only on the bottom of the container. Mixtures contain two different types of particles (shown here in different colors) which are not chemically bound.

The picture

pH units

The relative concentration of hydrogen ions in various body fluids is measured in concentration units

secondary structure

The second level of protein structure; the regular local patterns of coils or folds of a polypeptide chain.

tertiary structure

The third level of protein structure; the overall, three-dimensional shape of a polypeptide due to interactions of the R groups of the amino acids making up the chain.

What is the atomic symbol and mass number for an atom containing 50 protons and 64 neutrons?

Tin or Sn

Dipeptide

Two amino acids bonded together by a peptide bond

complementary bases

Two bases that pair together. A is complementary to T and C is complementary to G.

Isomers

Two different molecules that have the same chemical formula

predict the chemical formula for the ionic compound formed by v3+ and no2−

V(NO2)3

Rearrange the following equation to solve for V: PV= nRT

V= nRT/P

deoxyribonucleic acid

What does DNA stand for?

The element symbol for ytterbium is __

Yb

single covalent bond

a bond formed when two atoms share a pair of electrons

Orbital diagram

a diagram that shows the distribution of electrons in the orbitals of the energy levels

r group

a functional group that defines a particular amino acid and gives it special properties.

mixtures

a physical combination of substances that can still be seperated

decompisition reaction

a reaction in which a single compound breaks down to form two or more simpler substances. Ex fats are digested in your small intestine

neutralization reaction

a reaction in which an acid and a base react in an aqueous solution to produce a salt and water

displacement reaction

a reaction in which one element replaces a similar element in a compound. Ex. Glucose and ATP exchange to make Glucose phosphate and ADP

energy level

a region of an atom in which electrons of the same energy are likely to be found

active site

a region on an enzyme that binds to a protein or other substance during a reaction.

enzyme-catalyzed reaction

a substrate attaches to the active site. an enzyme-substrate (ES) complex forms. reaction occurs and products are released. an enzyme is used over and over.

Cysteine

a sulfur-containing amino acid that occurs in keratins and other proteins, often in the form of cystine, and is a constituent of many enzymes.

The number 7.13 × 10-5is equal to _______.

a)0.0000713

The measurement 127.3 is written in scientific notation as _________.

a)1.273 × 10^2

The measurement 420 000 m is written in scientific notation as _________. a)4.00×105 m b)4.25×104 m c)4.20×105 m d)4.25×105 m

a)4.20 ×105m

Where can you find chemicals?

a)In laboratory b)In grocery or hardware store c)All around you and inside you

arteriosclerosis

abnormal hardening of the walls of an artery or arteries

Oxidase

adds electrons to oxygen

Iodine-131

also known as radioiodine or radioactive iodine; a form of iodine use in medical diagnostics and treatments, e.g., to treat hyperthyroidism

electric current

ampere

weak acids

an acid that is only slightly ionized in aqueous solution ex. carbonate acid, acetic acid

hydrogen ion (H+)

an atom of hydrogen that has lost its electron

Triglycerides

an energy-rich compound made up of a single molecule of glycerol and three molecules of fatty acid.

neutral solution

any aqueous solution in which [H+] and [OH-] are equal ex. distilled water

oxidation-reduction reaction

any chemical change in which one species is oxidized (loses electrons) and another species is reduced (gains electrons); also called redox reaction. Ex. Sometimes this reaction changes the pattern of electron sharing in covalent bonds. The common factor in this these events is that electrons that formerly belonged to the reactant molecule either lost entirely or relatively.

Holoenzyme

apoenzyme + cofactor

Most matter changes

because of heat energy

amino acids

building blocks of proteins

Which of the following represents the numbers of protons and electrons in a bromide ion, Br-?.

c) 35p+and36e-

The name of the compound whose formula is CaBr2 is _______.

calcium bromide

The name of the compound Ca3(PO4)2 is ________

calcium phosphate

functional proteins

category of proteins that affect the functional operations of a cell; contrast to structural protein

fatty acids

chains of carbon atoms bonded to hydrogen atoms

Which of the following does not describe a mixture:, （a)properties of its components are retained,(b)chemical bonds are formed,(c)components can be separated physically,(d)includes both heterogeneous and homogeneous

chemical bonds are formed

carbonic acid-bicarbonate buffer system

chemical system that helps maintain pH homeostasis of the blood, carbonic acid(weak acid) dissociates reversibly, releasing bicarbonate ions(weak base) and protons

Hydrolases

cleave bonds on molecules with the addition of water

Lipoproteins

clusters of lipids associated with proteins that serve as transport vehicles for lipids in the lymph and blood

inorganic compounds

compounds that DO NOT contain carbon; Ex: Vitamins, minerals, water

acids

compounds that form hydrogen ions when dissolved in water Ex. hydrochloric acid

ketosis

condition resulting from uncontrolled diabetes mellitus, in which the body has an abnormal concentration of ketone bodies resulting from excessive fat metabolism

Eicosanoids

diverse lipids chiefly derived from a 20-carbon fatty acid found in all cell membranes

Hund's Rule

electrons occupy orbitals of the same energy in a way that makes the number of electrons with the same spin direction as large as possible

copper wire

element

Matter changes when

energy is added or taken away

ionizing radiation

enough energy to dislodge electrons from atoms, forming ions; capable of causing cancer (gamma, X-rays, UV)

Acidosis

excessive acidity of body fluids

fibrous proteins

extended and strand-like proteins, insoluble in water and very stable, used for tissues

saturated

fatty acid chains with only single covalent bonds between carbon atoms

Unsaturated

fatty acids that contain one or more double bonds between carbon atoms Ex. oils in cooking

In the process of making biofuel from corn, the corn is ground, mixed with water, and then enzymes are added to ferment the starch. The fermentation produces ethanol and carbon dioxide. The ethanol is further distilled for use as a biofuel. In this process ______ is an example of a chemical change

fermenting the starch

Steriods

flat molecules made of four interlocking hydrocarbon rings, fat soluble and contain little oxygen. Ex. Cholesterol in eggs, meat, cheese

Ocet Rule

for a stable atom, elements want to have 8 electrons in there valence shell

hydrocarbon chains

formed by successive bonds between carbon atoms and may be branched or unbranched. Makes neutral fats non-polar because polar and non polar molecules do not interact, oil and water do not mix

Fructose

fruit sugar- converted to glucose and metabolized

Carbon Dioxide (CO2)

gas (waste) released by body cells, transported via veins to the heart, and then to the lungs for exhalation. It is also a double bond where carbon is bonded by two oxygens. Oxygen being electronegative attracts to carbon on either side, rendering it a non-polar covalent bond.

Enzymes

globular proteins that act as biological catalysts, increases the speed of a reaction

Monosaccharides

glucose, fructose, galactose, single-chain structure containing three to seven carbon atoms

The name of the compound whose formula is AuCl3 is _______

gold() chloride

Radioisotopes

heavier Isotopes that have unstable nuclei and undergo radioactive decay. This occurs when alpha, beta or gamma particles are ejected from the atomic nucleus

A common laser relies on a mixture of He and Ne. What elements do these symbols represent?

helium and neon

coke

homogeneous mixture

true solution

homogeneous mixture of two or more substances able to pass through a semi-permeable membrane The size of the solute particles is less than one nanometer. Not visible to the naked eye, do not settle out, and do not scatter light

Calcium Nitrate

inorganic compound, colorless salt that absorbs moisture from the air, tetrahydrate shape

Which of the following elements is NOT represented by a single-letter element symbol?

iron

mass

kilogram (kg)

crystals

large arrays of cations and anions held together by ionic bonds

Polymers

large compound formed from combinations of many monomers Ex. starch and glycogen

ATP synthesis

large protein that uses energy from H+ ions to bind ADP and a phosphate group together to make ATP

half-life

length of time required for half of the radioactive atoms in a sample to decay

Which of the following is not an example of matter? a)Table salt b)Light c)Water d)Sand

light

Proteins

long chains of amino acids joined together by dehydration synthesis

Electropositivity

low electron-attracting power resulting in the tendency to lose valence shell electrons to other atoms. Examples, potassium and sodium.

luminous intensity

lumen

nucleic acids

macromolecules containing hydrogen, oxygen, nitrogen, carbon, and phosphorus

Which scientist is credited for coining the term 'radioactivity' for the spontaneous emission of particles or radiation from atoms?

marie curie

What are some common ionic bonds that occur between elements?

metallic elements such as sodium, calcium and potassium with one or two valence electrons bond with elements such as chlorine, fluorine, and iodine with seven valence electrons.

What is the unit of length in metric system?

meter

length

meter (m)

Galactose

milk sugar

Phospholipids

modified triglycerides, where one fatty acid has been replaced with a phosphate group.

non-polar molecule

molecule that shares electrons equally and does not have oppositely charged ends

polar molecule

molecule with an unequal distribution of charge, resulting in the molecule having a positive end and a negative end

amphipathic

molecules that have both polar and nonpolar parts

molarity

moles of solute/liters of solution

Nucleotide

monomer of nucleic acids made up of a 5-carbon sugar, a phosphate group, and a nitrogenous base

bicarbonate ion

most important buffer in human blood

Rutherford's gold foil experiment determined that

most of the space in an atom is empty except for a concentrated area called the nucleus. Solution:

anion

negatively charged ion (gained electrons)

Paul exclusion principle

no two electrons in the same atom can have the same set of four quantum numbers

Monoatomic elements

noble gases, Au

Avogadro's number

number of representative particles in a mole, 6.02 X 10^23

one molar solution

one mole of solute dissolved in water to make 1 liter of solution

amine group

organic compounds and functional groups that contain a basic nitrogen atom with a lone pair

quarks

particles of matter that make up protons and neutrons, less effective in heavier isotopes

Any melting or freezing points are

physical property

Which set of terms best describes a proton?(a)nega- (b)positive charge, l amu,in the nucleus;(c)uncharged,1 amu,in the nucleus

positive charge, l amu,in the nucleus

ions

positively and negatively charged atoms

cation

positively charged ion (lost electrons)

Apoenzyme

protein portion of an enzyme

biological colloids

protein- water mixtures, (ex) blood plasma and cerebrospinal fluid.

structural proteins

proteins that form an organism's physical attributes

atomic weight

protons + neutrons, atomic weight of an element is approximately equal to the mass number of its most abundant isotope.

alpha emission

radioactive decay of a nucleus that is accompanied by emission of alpha particles, lowest penetrating power towards tissue

spectroscopic notation

shorthand representation of the principal (n) and azimuthal (l) numbers Principal number remains a number Azimuthal number is designated by a letter l=0 subshell is called s; Group 1-2 plus helium, 1s^1-7s^2 l=1 subshell is called p; Group 3-8 minus helium 2p^1-7p^6 l-2 subshell is called d; middle gap 3d^1- 6d^10 l-3 subshell is called f; bottom two rows 4f^1-5f^14 s, p, d, f suk, pusy, dik, fuk example; electron in shell n=4 and subshell l=2 is said to be in the 4d subshell

Which of the following sets of elements and symbols is paired incorrectly?

silver Si

Gylcine

single H atom in side chain, small enough to fit into tight corners in a protein molecule

What fundamental force is responsible for holding together the subatomic particles of an atomic nucleus?

strong nuclear force

solutes

substances present in smaller amounts

The name of the compound SO3 is ________

sulfur trioxide

What is the place value of the 3 in the number 25.3?

tenths

mole

the SI base unit used to measure the amount of a substance

What happens when the atom's outermost shell is filled to capacity?

the atom becomes stable, chemically inert which is unreactive. Examples, noble gases such as helium, and neon

chemical bonds

the attractive forces that hold atoms together

electroneutral

the carbon never loses or gains electrons instead they always share them

surface tension

the force that acts on the surface of a liquid and that tends to minimize the area of the surface. Explains why water beads up on spheres when it sits on surface structures

gram molecular weight

the mass of a substance equal to its molecular weight in grams

Thymine

the nucleotide that hydrogen bonds with the nucleotide adenine in DNA.

chemical reaction

the process by which one or more substances change to produce one or more different substances

Carbohydrates

the starches and sugars present in foods, ex. Carbon, hydrogen, and oxygen use little for structural purposes such as sugars that are found in the genes. When protein intake is low, the liver converts sugars into building blocks needed to produce protein

Solvent

the substance present in the larger amount

globular proteins

these are compact, generally rounded, and soluble in water, chemically active molecules.

What is the place value of the 8 in the number 2.378?

thousandths

tripeptide

three amino acids bonded together

sol-gel transformations

to change reversibly from a fluid (sol) state to a more solid (gel) state

1 cc is the unit of what quantity?

volume

universal solvent

water

hydration layers

water forms layers of molecules around large charged molecules such as proteins, shielding them from the effects of other charged substances in the vicinity and preventing them from settling out of solution; protein-water mixtures are biological colloids; blood plasma and cerebrospinal fluid

buffers

weak acids or bases that can react with strong acids or bases to prevent sharp, sudden changes in pH

silver get oxidized

when it is exposed to air or moisture.