Chemistry: Lecture 1: Atoms, Molecules, And Quantum Mechanics

Front 1

What is the mass of a proton/neutron?

Back 1

1 amu

Front 2

Mass Number

Back 2

A = protons + neutrons

Front 3

Atomic Number

Back 3

Z = protons

Front 4

Isotopes

Back 4

-Two or more atoms of the same element that contain different numbers of neutrons
-Isotopes have similar chemical properties

Front 5

amu

Back 5

-Atomic Mass Unit
-One atom of carbon 12 has an atomic weight of 12 amu
-6.022*10^23 amu = 1 gram

Front 6

Mole

Back 6

6.022 * 10^23

-The number of carbon atoms in 12 grams of carbon 12

Front 7

Period

Back 7

Horizontal rows

Front 8

Groups/Families

Back 8

Vertical columns

Front 9

Metals

Back 9

-Form cations(+)
-Metallic character includes ductility, malleability, thermal and electrical conductivity, and a characteristic luster
-Typically form ionic oxides

Front 10

Nonmetals

Back 10

-Form anions(-)
-Have lower melting points than metals
-Form covalent oxides

Front 11

Metalloids

Back 11

-Have some characteristics that resemble metals and some that resemble nonmetals

Front 12

Elements in the same ________ on the periodic table have similar chemical properties(tend to make same # of bonds, similarly charged ions)

Back 12

Family/Group

Front 13

Group 1A

Back 13

-Alkali Metals (form 1+ cations)
-Soft metallic solids with low densities and low melting points
-Highly reactive
-In nature, exist only in compounds

Front 14

Group 2A

Back 14

-Alkaline Earth Metals (form 2+ cations)
-Harder, more dense, and melt at higher temperatures than alkali metals

Front 15

Group 5A

Back 15

-Can form 3 covalent bonds
-All 5A elements except nitrogen can form five covalent bonds by using d orbitals
-Nitrogen(strong) and Phosphorus(weak) can form pi bonds

Front 16

Group 6A(chalcogens)

Back 16

-Includes oxygen and sulfur

Front 17

Oxygen

Back 17

-Second most electronegative element
-Divalent and can form strong pi bonds

Front 18

Sulfur

Back 18

-Can form 2,3,4, or even 6 bonds
-Has ability to make strong pi bonds

Front 19

Group 7A(halogens)

Back 19

-Highly reactive (like to gain e-)
-Fluorine always has oxidation state of -1, meaning it only makes one bond

Front 20

Noble Gases

Back 20

-Nonreactive
-All gases at room temperature

Front 21

Small Atoms

Back 21

-Bond strongly to water, resulting in greater heats of hydration
-Don't have d orbitals, so can't form more than 4 bonds
-Make strong pi bonds due to overlap of p orbitals

Front 22

Large Atoms

Back 22

-Have d orbitals allowing for more than 4 bonds
-Unable to make strong pi bonds

Front 23

When the transition metals form ions, they lose electrons from their ____ subshell first, and then from their ____ subshell

Back 23

s,d

Front 24

How do atoms lose electrons?

Back 24

Atoms lose electrons from the highest energy shell first

Front 25

Isoelectric Ions

Back 25

-Ions with the same number of electrons
-Tend to get smaller with increasing atomic #

Front 26

Effective Nuclear Charge(Zeff)

Back 26

-The amount of charge felt by the second electron (EX: in helium)
-Increases from left to right and top to bottom

Front 27

Ionization Energy

Back 27

-The energy necessary to detach an electron from a nucleas
-Increases from left to right and bottom to top

Front 28

Electronegativity

Back 28

-Tendency of an atom to attract an electron in a bond that it shares w/ another atom
-Increases from left to right and bottom to top

Front 29

Electron Affinity

Back 29

-The willingness of an atom to accept an additional electron (energy that is released when an electron is added to a gaseous atom)
-Increases from left to right and bottom to top

Front 30

Atomic Radius

Back 30

-Increases from right to left and top to bottom

Front 31

Metallic Character

Back 31

-Increases from right to left and top to bottom

Front 32

Bond Length

Back 32

-Defined as the point where the energy level is the lowest

Front 33

Compound

Back 33

-A substance made from two or more elements in definite proportions

Front 34

T or F: Energy is not always required to break a bond

Back 34

F

Front 35

T or F: No energy is ever released by breaking a bond

Back 35

T

Front 36

Crystalline Solids

Back 36

-Sharp melting point, characteristic shape w/ a well ordered structure of repeating units (atoms, molecules, or ions)
-Can be ionic, network covalent, metallic, or molecular

Front 37

Amorphous Solid

Back 37

-Has no characteristic shape and melts over a temperature range (EX: glass)

Front 38

Polymers

Back 38

-Solids w/ repeated structural units, and can be crystalline or amorphous
-Rapid cooling results in amorphous solids
-Slow cooling results in crystalline solids

Front 39

First Quantum Number

Back 39

-Designates the shell (n)
-Has the value (n)

Front 40

Second Quantum Number

Back 40

-Designates the subshell (l): s,p,d, and f
-Ranges from zero to n-1

Front 41

Third Quantum Number

Back 41

-Designates the orbital (ml)
-Ranges from l and -l

Front 42

Fourth Quantum Number

Back 42

-Designates the spin (ms)
-Ranges from 1/2 to -1/2

Front 43

Heisenberg Uncertainty Principle

Back 43

dx*dp = h

Front 44

Hund's Rule

Back 44

-Electrons will not fill any orbital in the same subshell until all orbitals in that subshell contain at least one electron, and the unpaired electrons will have parallel spins

Front 45

Planck's Equation

Back 45

dE = hf (f = frequency)

Front 46

de Broglie Equation

Back 46

wavelength = h/mv