The Nature of Molecules & The Property of Water (CH 2)

Question 1

How do you determine the Atomic Number?

Answer 1

-Same number of Protons

Question 2

How do you determine Atomic Mass?

Answer 2

-Protons + Neutrons

Question 3

What’s the Mass of each Subatomic Particle?

Answer 3

• Protons= 1 Dalton
• Neutrons= 1 Dalton
• Electrons= 1/1840 Daltons

Question 4

What are Atoms?

Answer 4

-Interacting Subatomic Particles

Question 5

What are Molecules?

Answer 5

-Interacting Atoms

Question 6

What are Cells?

Answer 6

-Interacting Molecules

Question 7

What are Organisms?

Answer 7

-Interacting cells

Question 8

What is Special Relativity?

Answer 8

• ALL physical laws (including speed of light) MUST BE THE SAME to all observers
• Everything that we think of as “constant” MUST CHANGE= Length, mass, time
• EX; if distance appears longer to observer B than observer A , time must get longer in order for the speed of light to remain constant

Question 9

What are Ions?

Answer 9

-Atoms where # of electrons is not equal to the # of protons

Question 10

What is a Cation?

Answer 10

• Atoms where the # of protons is greater than the # for elections
• Atom with 1 electron in their outer shell will lose on electron easily= release a ton of energy

Question 11

What is an Anion?

Answer 11

• Atoms where the # of elections are greater than the # of protons
• Atoms with 7 electrons in their outet shell will gain one easily & dangerously

Question 12

What is an Isotope?

Answer 12

-Atoms of a single element that have different # of electrons

Question 13

What are Radioactive Isotopes?

Answer 13

• Have constant decay rate
• Decay time= Half Life bc of the time it takes for 1/2 an atom to decay
• Makes good tracers/ tags to follow specific molecules progress of chemical reactions/living in cells or tissue

Question 14

What are the 4 forces?

Answer 14

• Gravity
• Weak Nuclear Force
• Electromagnetism (between atoms & molecules= chemical bonds)
• Strong Nuclear Force

Question 15

What are Hadrons?

Answer 15

• Heavy Particles
• Protons, neutrons, other
• NOT elementary bc made up of quarks
• 2 types= Bayrons & Mesons

Question 16

What are the 2 Properties of Quarks?

Answer 16

• Mass of a proton/ neutron is 100x larger than mass of component quarks, neutrons= 1% while PE & KE is 99%
• Quarks can’t be separated from eachother= the more you pull them apart, the more they’re attracted to each other. They also don’t break up when you try to blow them apart

Question 17

What is Energy Minimization?

Answer 17

• Total energy & PE of a system will ALWAYS go to the MINIMUM
• Releases energy via favorable reactions that occur but doesn’t gain energy via unfavorable reactions

Question 18

How are Ionic Bonds formed?

Answer 18

• When ions of an opposite charge attract eachother
• It is an Energetic tendency
• Ionic compounds= crystalline solids (NaCl) ALWAYS form into cubes. Na Ion loses electron= Oxidation (+1), Cl gains electron= Reduction (-1)

Question 19

What are Bosons?

Answer 19

• Elementary particle
• Carries fundemental forces
• Photons= mediate electromagnetism
• Gluons= mediate strong force

Question 20

What is Quantum Mechanics?

Answer 20

• Interactions between matter & energy are discrete (quantized) & not continuous at a microscopic scale
• Have to add integer to energy NOT DECIMALS

Question 21

How many Daltons are in a gram?

Answer 21

-6.02x10^23 daltons

Question 22

What are the 3 Elementary particles?

Answer 22

• Quarks
• Leptons
• Bosons

Question 23

What are Leptons?

Answer 23

• Lighter particles

- Have -1 charge

Question 24

What are Quarks?

Answer 24

• Make up protons and neutrons
• Up Quark= charge of +2/3e
• Down Quark= charge of -1/3e

Question 25

How are Chemical Bonds made?

Answer 25

-Electromagnetic forces between atoms & molecules

Question 26

What is a Mol?

Answer 26

• Unit amount of a substance
• 1mol= 6.02x10^23 particles
• Conversion between atomic mass & grams

Question 27

How big is the Nucleus of an atom?

Answer 27

• 100 fold SMALLER than electron shell

- If nucleus was a golf ball, an electron would be a mile away

Question 28

What are Electron Orbitals?

Answer 28

• VOLUMES where an electron may be statistically located
• Only a max of 2 electrons allowed per orbital
• Filled from lowest to highest energy
• Filling of orbitals determine property & chemical reactivity
• S orbitals (left side)= Spherical vs L orbitals(right side) are elongated
• First row of Periodic table fills S orbital & then P orbital for outermost shell

Question 29

What are Electron Shells?

Answer 29

• Energy levels= One or more orbitals that have the same energy
• Start with K=1 and so on
• Outer shell= Valience shell= most reactive & largely detemines chemistry

Question 30

How do the rows with Langthinides and Actinides and Transition metals fill in Electron Orbitals?

Answer 30

• Fill in NON outermost shell= have less effect on relativity
• Filling D orbitals= 1 down of the most outermost shell
• Lang & Act fill F orbitals which are 2nd from outermost shell (6th row but is 4F)

Question 31

What are Valience Electrons?

Answer 31

• Are at the outermost shell= Valience Shell

- Most acessible to other atoms & electromagnetic force

Question 32

What can you tell from the Columns of the Periodic Table?

Answer 32

• Each is a group= have SAME # of electrons in outershell= similar chemical properties
• Columns w/ partially filled electron shells= reactive
• Next to last column on right= Electron that need to be added to complete shell
• Last column on left= shell that needs to lose electron

Question 33

What two things are ALWAYS associated with eachother?

Answer 33

-Mass & energy!

Question 34

What is Oxidation?

Answer 34

-Losing an electron to another atom

Question 35

What is Reduction?

Answer 35

-Adding electron to atom’s orbital

Question 36

Where is Methylene found?

Answer 36

-In the middle of molecules

Question 37

What does water do?

Answer 37

-Spontaneously ionizes into H+ & OH- ions