Unformatted text preview:

BSC2010 – FINAL EXAM REVIEWChapter 2 – The Basics*- Matter : anything that takes up space and has mass- Element : a substance that cannot be broken down to other substances by chemical reactiono 20-25% of elements are essential to lifeo Most abundant elements in the human body: carbon (18.5%), hydrogen (9.5%), oxygen (65%), nitrogen (3.3%), and calcium (1.25%)o Trace elements : required by an organism in minute quantitieso Properties of an element: neutrons (no charge), protons (positive charge), electrons (negative charge)- Compound : substance consisting of two or more elements in a fixed ratio- Atom : smallest unit of matter that still retains the properties of an element- Atomic mas s = proton mass + neutron mass- Mass number = amount of protons + amount of neutrons- Isotopes : atoms of an element that differ in the number of neutronso Radioactive isotopes: decay spontaneously, giving off particles and energyo Uses of radioactive isotopes: dating fossils, tracing atoms through metabolic processes, diagnosing medical disorders- Energy : capacity to cause changeo Potential energy: energy that matter has because of its location of structureo Kinetic energy: energy of motion- An electron’s state of potential energy is called its energy level, or electron shello the outermost electron shell determines chemical reactions/bonds that can occuro valence electrons: those in the outermost shell (valence shell)- Orbital : 3D space where an electron is found 90% of the time- Molecule : 2 or more atoms held together by covalent bonds, smallest unit of a compound that retains the properties of a compound- Solution : compound in a homogenous suspension- Solvent : dissolving medium- Solute : dissolved substance- Molecular formula : gives the type of atoms in a compound and the number of each type; ex. H2- Structural formula : gives more detailed chemical formula that shows bonds between atoms; shows how atoms are arranged; ex. H – H - Covalent bond : sharing of a pair of valence electrons by two atoms ,the shared electrons count as part of each atom’s valence shello Single bond: sharing one pair of electronso Double bond: sharing two pairs of valence electronso Nonpolar covalent bond: atoms share electrons equallyo Polar covalent bond: one atom is more electronegative and the atoms do not share the electrons equally (unequal sharing of electrons causes a partial positive or negative charge for each atom or molecule)- Electronegativity : an atom’s attraction for the electrons in a covalent bond; the more electronegative an atom, the more strongly it pulls shared electrons to itself- Ions : electrically charged atomso Anion: negatively charged iono Cation: positively charged ion- Ionic bond : attraction between an anion and a cation (form salts)- Hydrogen bond : forms when a hydrogen atom covalently bonds to one electronegative atom that is also attracted another electronegative atom- Van der Waals interactions : attractions between molecules that are close together as a result of “hot spots” of positive or negative charge thatcauses asymmetrical distribution- Diffusion : spontaneous movement of molecules; molecules move down a concentration gradient- Chemical reactions : collisions between molecules can lead to rearrangement of electrons between orbitals. Making and breaking of bonds andformation of new compounds is a chemical reaction.- Equilibrium : when forward and reverse reactions occur at the same rateo All chemical reactions are reversible-products of the forward reaction become reactants for the reverse reactionChapter 3* - There are four critical properties of water1. Cohesion/Adhesion 1. Cohesion: hydrogen bonds hold water molecules together; helps the transport of water against gravity in plants2. Surface tension: measure of how hard it is to break the surface of a liquid3. Adhesion: attraction between different substances, for example, between water and cell walls2. Moderation of Temperature 1. Water absorbs heat from warmer air and releases stored heat to cooler air2. Water can absorb or release a large amount of heat with only a slight change in its own temperature3. Kinetic energy: energy of motion4. Heat: measure of total kinetic energy due to molecular motion5. Temperature: the intensity of heat due to the average kinetic energy of molecules6. Calorie: the amount of heat required to raise the temp. of 1 g or water by 1 degree Celsius; 1kcal=1000cal; 1cal=4.184J7. Specific heat: amount of heat that must be absorbed or lost for 1 g of that substance to change its temperature by 1 degree Celsius  Water has an extremely high specific heat8. Evaporation: transformation of a substance from liquid to gas9. Heat of vaporization: heat a liquid must absorb for 1 g to be converted to gas3. Density 1. Water reaches its greatest density at 4 degrees Celsius2. Ice floats in water because hydrogen bonds in ice are more “ordered,” making ice less dense 3. Solution: a liquid that is a homogenous mixture of substances4. Solvent: dissolving agent of a solution5. Solute: substance that is dissolved6. Aqueous solution: solution in which water is the solvent4. Water is a versatile solvent 1. Forms hydrogen bonds easily2. Hydrogen shell: sphere of molecules that surround each ion of an ionic compound dissolved in water3. A hydrophilic substance is one that has an affinity for water.4. A hydrophobic substance is one that does not have an affinity for water.5. Molecular mass: sum of all masses of all atoms in a molecule6. Avogadro’s number = 6.02 x 1023Acids and Bases- A hydrogen atom in a hydrogen bond between two water molecules can shift from one to the othero The hydrogen atom leaves its electron behind and it transferred as a proton, or hydrogen ion (H+)o The molecules with the extra proton is now a hydronium ion (H3O+), though it is often represented as H+o The molecule that lost the proton is how a hydroxide ion (OH-)- Acid : any substance that increases the H+ concentration of a solution- Base : any substance that reduces the H+ concentration of a solution- pH : negative logarithm of H+ concentration –log[H+]o determines how acidic or basic a solution iso >7 basic, <7 acidic, =7 neutralo Most biological fluids have a pH of 8- Buffers : substances that minimize changes in concentration of H+ and OH- in a solution- Ocean acidification : when CO2 dissolves in seawater to create carbonic acid-


View Full Document

FSU BSC 2010 - FINAL EXAM

Documents in this Course
Notes

Notes

1 pages

Notes

Notes

1 pages

Notes

Notes

1 pages

Notes

Notes

1 pages

Notes

Notes

2 pages

Notes

Notes

1 pages

Unit 1

Unit 1

8 pages

Chapter 1

Chapter 1

10 pages

EXAM 2

EXAM 2

7 pages

Notes

Notes

1 pages

Test 1

Test 1

35 pages

ATOMS

ATOMS

6 pages

Notes

Notes

1 pages

Notes

Notes

1 pages

Notes

Notes

7 pages

Notes

Notes

1 pages

Test 4

Test 4

36 pages

Notes

Notes

1 pages

Notes

Notes

1 pages

Test 1

Test 1

24 pages

Exam 4

Exam 4

28 pages

Test 1

Test 1

20 pages

Test 1

Test 1

21 pages

Notes

Notes

1 pages

Chapter 1

Chapter 1

131 pages

Chapter 1

Chapter 1

131 pages

Chapter 1

Chapter 1

66 pages

Exam 3

Exam 3

25 pages

Exam 3

Exam 3

25 pages

Exam 3

Exam 3

19 pages

Exam 2

Exam 2

22 pages

Exam 3

Exam 3

27 pages

Exam 3

Exam 3

27 pages

Exam 2

Exam 2

10 pages

Exam 2

Exam 2

29 pages

Exam 2

Exam 2

29 pages

Test 1

Test 1

20 pages

Test 4

Test 4

11 pages

Exam 5

Exam 5

46 pages

Oxidation

Oxidation

30 pages

LESSON 8

LESSON 8

16 pages

Test 1

Test 1

37 pages

Exam 3

Exam 3

17 pages

Chapter 1

Chapter 1

14 pages

Exam 1

Exam 1

4 pages

Exam 3

Exam 3

23 pages

Exam 2

Exam 2

8 pages

Exam 3

Exam 3

8 pages

Exam 3

Exam 3

27 pages

Exam 4

Exam 4

8 pages

Topic 5

Topic 5

3 pages

Load more
Download FINAL EXAM
Our administrator received your request to download this document. We will send you the file to your email shortly.
Loading Unlocking...
Login

Join to view FINAL EXAM and access 3M+ class-specific study document.

or
We will never post anything without your permission.
Don't have an account?
Sign Up

Join to view FINAL EXAM 2 2 and access 3M+ class-specific study document.

or

By creating an account you agree to our Privacy Policy and Terms Of Use

Already a member?