Unit 1 Bio 180

Front 1

What is a Element?

Back 1

Element cannot be broken down to other substances by chemical recations

"basic building blocks of the universe"

Matter that can no longer be broken down

Front 2

How many natural occuring Elements?

Back 2

92

Front 3

4 elements that make up 96% of living matter

Back 3

Carbon, Oxygen, Nitrogen, Hydrogen

Hint 3

"Heck no" (HCNO)

Front 4

Compound

Back 4

substance consisting of 2 or more elements

Front 5

A)what is a Atom?

B)What are the 3 parts of a Atom

Back 5

a)smallest partical of a element that keeps all of its properties

partical of a element that keeps all of its properties

b) Proton, Neutron, Electron

Front 6

Properties of a Proton

i. Charge?

ii. where located

iii. Weight

iiiiDetermines what? (2)

Back 6

i.Positive chargeii.Found in nucleusiii.~1 Dalton or atomic mass unit)iv.Determines mass, determines element

Front 7

Properties of a Neutroni. Charge?ii. where locatediii. WeightiiiiDetermines what? (2)

Back 7

i.No charge

ii.Found in nucleusiii.~1 Dalton or atomic mass unit)iv.Determines mass, determines isotope

Front 8

Properties of a Electroni. Charge?ii. where locatediii. WeightiiiiDetermines what? (2)

Back 8

i.Negative chargeii.~1/2000 mass of proton or neutroniii.Found in electron cloudiv.Determines chemical behavior and bonding properties, determines charge

Front 9

Atomic Number

What is the symbol?

Back 9

Number of Protons in Nucleus (also number of electrons

Z

Front 10

Mass Number

What is the symbol

Formula for how many neutrons in a atom?

Back 10

Sum of Protons and Neutrons in nucleus

A

Mass number- Atomic number= Neutrons

Front 11

a)Isotopes

b)What is the most common Isotope?

Back 11

a)Atoms with the same atomic number but different mass numbers (more or less neutrons)

b) Carbon-12,, carbon-13, carbon-14

Front 12

Weight of a Proton

Back 12

1 dalton or 1 AU

Front 13

1-What is a ion?

2- What are the two types of ions and properties?

Back 13

1-atom with more or less electons than protons

2a- Cation =positive ion (less electrons)

2b- Anion= Negative ion (more electrons)

Front 14

1-Mole

2-What is Avagadro's number

Back 14

1-How many of a certian atom can fit in a gram?

2- 6.02x10^23

Front 15

Ratioactive Isotopes

Back 15

Atoms with unstable nucli

Front 16

1-Ratioactive decay

2- 3 types of decay and prperties

i)what is emmitted

ii)mass and velocity

iii)nuclear effect

3- List in order of lease distructive to most distructive

Back 16

1-Ratioactive isotope becoming balanced through emission of Particles and Light

2a- Alph Particle- i.Helium Nucleus (2p + 2n), ii.high mass, low velocity, iii.Nuclear effect A=-4 Z=-2

2b- Beta Particle- i.Electron(high energy) Low mass, high velocity iii. A=0 Z=+1

2c- Gamma Particle- i Energy wave ii. No mass, high velocity. iii. no effect

Front 17

Ratioactive Isotopes properties (4)

Back 17

1. Easily Detectable

2.Reacts the same as a stable isotope

3. Damage proteins and DNA cells ( what is the order from least to most distructive)

4.constant, predictable decay

Front 18

Half Life

Back 18

amount of time required for half of a ratioactive smaple to decay

Front 19

Half life formula and what each part mean

Back 19

N= (No)e^-0.693T/(T1/2)

N= Amount of radioactivity after T

No= Starting amount of ratioactivity

T= amount of time sample decay

T1/2= Half life

Front 20

Ratioactive dating

Back 20

Scientist determining how long something has been dead by tracking radiation

Front 21

Molecule

Back 21

2 atoms covalently bound togther (can be same or different

Front 22

Compound

Back 22

combination of 2 or more elements

Front 23

What is the Bohr Model

Back 23

Drawing of the nucleus and the electons in circles around the nucleus

Front 24

Quantum Model

Back 24

Replaced the bohr model to show the duel nature of electrons (wave and particle)

Front 25

Electromagnetic wave

Back 25

1.Form of traveling energy, formed by oscillating electrical and magnetic waves2.Spectrum of different waves. Includes gamma rays, x-rays, ultraviolet & visible light, infrared, microwave, and radio waves3. Each wave is defined by its wavelength4.Smaller wavelengths carry more energy

Front 26

Absorbance

Back 26

Absorbance–the conversion of a specific wavelength of light into energy need to excite anelectron to ahigher shell. Color results from selective absorption of light

Front 27

Excitation

Back 27

Excitation–movement of an electron from its ground state to a higher energy shell. Aquantum process, meaning only a specific wavelength is accepted.

Front 28

Relaxation

Back 28

Relaxation–movement of an electron from an excited state back to its ground state. Energyis emitted as a result

Front 29

Floresence

Back 29

Fluorescence–emission of light waves from relaxing electrons. Causes ‘day-glo” colors.Emission wavelength is typically longer wavelength/lower energy than absorbedwavelength

Front 30

4 types of Light/ electron interactions

Back 30

Aborbance, Excitation, Relaxation, Floresence

Front 31

Quantum Model- Model Features

Back 31

Quantum Model–A.Model Features1.Electrons can’t “orbit” the nucleus2.Electrons behave as particles and as waves3.Based on wave probability formulas called wave functions4.Electrons reside in an orbital

Front 32

Quantum model- orbitals

Back 32

B.Orbitals1.Probability of where an electron is 95% of time2.Come in different shapes and sizes according to energy level3.Each orbital can hold a maximum of 2 electrons4.Lower energy orbitals fill with electrons before higher energy orbitals are occupied5.Orbitals at the same energy level are each occupied with oneelectron before any fill with two

Front 33

Quantum Orbitals- Organization levels

Back 33

Organization levels–the following are represent both physical space and energy levels1.Shells (like buildings)2.Subshells (like floors)3.Orbitals (like rooms)4.Spin (like beds)

Front 34

how does Eletromagnetic raditaion travel

Back 34

Waves

Short wave-more energy

Long Wave-less energy

Front 35

According to the Quantum model, how does electrons move

Back 35

Move both as a wave and a particle

Front 36

1-What order are the subshells labeled

2-How many orbitals does each subshell hold

3- How many electrons are in each orbital

Back 36

1-s,p,d,f

2- s(1), p(3),d(5),f(7)

3- 2 electrons

Front 37

Write the electron configuration for the following elements

1. O A=8

2. Cl A=17

3. Ag A= 47

Back 37

1. 1s^2, 2s^2, 2p^4

2. 1s^2, 2s^2, 2p^6, 3s^2, 3p^5

3. 1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 4s^2, 3d^10, 4p^6, 5s^2, 4d^9 (short hand [Kr], 5s^2, 4d^9)

Front 38

Octet Rule

Back 38

Atoms acting in a way to fill their outer valance shell (example Ionization and Bonding)

Front 39

Draw the lewis dot structure for the following atoms

1. C

2. S

3. Mg

4. Ar

Back 39

1. 4 dots around

2. 6 dots around (2 pairs)

3. 2 dots around

4. 8 dots around (4 pairs)

Front 40

Why are noble gases stable

Back 40

They have a full valence shell

Front 41

what shape does a sp3 Hybrid orbitals

Back 41

Tetrahedral

Front 42

what are two ways a non- noble atom can achieve an octet of electrons

Back 42

Atom giving up or gaining a new electron.

Covalent bonding

Ionization

Front 43

covalent bonding

Back 43

-sharing of unpaired electrons between two atoms

-strong bond 100-300 kj/mol

Front 44

what are the two types of covalent bonding? what are their properties?

Back 44

Polar covalent bond- unequal sharing of electrons (partial positive and negative charges)

Non- polar covalent bond- equal sharing of electrons

Front 45

Electronegativity

What is the pattern on the Periodic table for electronegativity

Back 45

how much a atom want to fill its valence shell. (ask for me to explain)

Front 46

Polar vs nonpolar vs ionic scale or

electronegative scale

Back 46

Nonpolar 0- 0.4 (equal charges)

Polar 0.4-1.7 (partcial charges)

Ionic 1.8 and more (not sharing electrons)