Flip Me Over
Ok, so Iām too lazy to type these up, but ya gotta know the first 36 elements and their symbols and whatnot AND also Ag, Au, Pb, Hg, I
okie dokie? okie dokie.
Elements
Pure substances from which all other things are build
Made up of 1 atom
Cannot be broken down further
Chemical Symbols
Represent the names of the elements
Consist of 2 symbols
One uppercase, one lowercase
*spelling counts*
What is Zn?
Aluminum or Aluminium?
Flourine or Fluorine?
Zinc
Aluminum
Fluorine
Periodic Table
Organizes 118 elements into groups with similar properties and places them in order of increasing atomic number
Groups
Contain elements with similar properties in vertical columns
Also called families
Periods
Horizontal rows of elements counted from top to bottom as periods 1-7
How are groups labeled?
Old Naming:
A = representative elements (Main Group)
First 2, and Last 6
B = transition elements
10 in the Center
New Naming:
All columns are labeled left to right 1-18
What are the sections and families of the period table?
1A (1) = Alkali Metals
2A (2) = Alkaline Earth Metals
The Bs (3-12) = Transition Metals
7A (17) = Halogens
8A (18) = Noble Gasses
Hydrogen = broās weird, has its own section
Alkali Metals
Extremely reactive
Stored in oil bc water will make them react
Group 1A
Lithium (Li)
Sodium (Na)
Potassium (K)
Rubidium (Rb)
Cesium (Cs)
*as you go down the list, the reactivity increases*
Alkaline Earth Metals
Shiny + not as reactive as 1A
Used in fireworks!
Group 2A
Beryllium (Be)
Magnesium (Mg)
Calcium (Ca)
Strontium (Sr)
Barium (Ba)
Radium (Ra)
Halogens
Toxic, smell bad, reactive and form compounds with most of the elements
Especially with 1A
Group 7A
Fluorine (F)
Chlorine (Cl)
Bromine (Br)
Iodine (I)
Heavy Zigzag
Separates nonmetals and metals
Metals: on the left
Non-Metals: on the right
Metalloid: along the zigzag (not alumnium)
Metals
Shiny
Ductile (ability to be pulled into wires)
Conduct heat and electricity
Solid at room temp (except Mercury)
High densities and melting points
Why is hydrogen not included with the metals?
It displays more traits of nonmetals
Nonmetals
Dull
Brittle (becomes powder if tried to pull)
Poor conductors
Good insulators
Low densities and melting points
Metalloids
Exhibit properties of both metals and nonmetals
Better conductors than nonmetals but not as good as metals
Used as semi-conductors and insulators
They can be modified to function as conductors or insulators
Batteries, paints, ceramics, etc.
Atom
Smallest part of an element that maintains the characteristics of that element
What was Daltonās Atomic Theory also influenced by?
The Law of Conservation of Mass
Daltonās Atomic Theory
Atoms are tiny particles of matter
Atoms of one element are similar to each other and different from those of other elements
Atoms of two or more different elements combine to form compounds
Atoms are rearranged to form new combinations in a chemical reaction
What are the subatomic particles and what are their charges?
Protons = positive; pāŗ
Electrons = negative; eā»
Neutrons = neutral; nā°
Like charges _____ , unlike charges ______
Like charges repel, unlike charges attract
Atoms are always neutral: True or False
True; elements and atoms are not the same, atoms must always be neutral
J.J. Thomsonās Cathode Ray
Realized that cathode rays contain negatively charged particles
Particles (now called electrons) have a much smaller mass than the atom
What did J.J. Thomson propse?
A āplum puddingā model; electrons were scattered randomly through a positively charged space
No knowledge of protons; just that there was positive charges
Rutherfordās gold foil
ā wanted to figure out how much space electrons took up
Positively charged particles were aimed at atoms of gold
Mostly went straight through, deflected only occasionally
Concluded that there must be a small, dense, positively charged nucleus that deflected the positive particles that came close to the nucleus
Atomic Structure
Nucleus in the center w/ protons and neutrons
Electrons that occupied the large empty space around the nucleus
Where is most of the mass of an atom?
The nucleus
Atomic Number
Appears above the symbol
Same for every atom of that element
The number of protons
A whole number
What does net 0 mean and what does that describe about the subatomic particles?
Net 0 = neutral
Same amount of protons and electrons
Mass Number
Located under the symbol
Not on our given periodic table :<
Represents the number of particles in the nucleus (protons and neutrons)
Isotopes
Different atoms of the same element
Have different mass numbers
The same number of protons, different number of neutrons
Can be distinguished by their atomic number
Ā²ā“Mg = the 24 is the mass
Do all isotopes occur in the same percentage?
Nope; they have varying ranges of occurrence
Formula for Calculating Atomic Mass of multiple Isotopes
For each isotope: Mass(amu) x percent abundance/100
Add up all the values (donāt forget sig figs)
If you are given ā¶L and ā·L and the mass given on the periodic table is 6.941 amu, which isotope is more abundant?
Since the 6 and 7 in ā¶L and ā·L represent the mass, and the value we are given is 6.941, we need to figure out which value is closer.
The more abundant something is, the more it will appear overall, itās the same principle with numbers. Meaning, we can use 6 and 7 as a range and since 6.941 is closer to 7, we can assume that ā·L is more abundant
Electromagnetic Radiation
Consists of energy particles that move as waves of energy
In different forms such as light, rainbow, x-ray
Distance between the peaks of waves
Wavelength
High-energy radiation has _____ wavelengths and low-energy has ______ wavelengths
High-energy radiation has short wavelengths and low-energy has long wavelengths
Electromagnetic Spectrum: Low to High
Radio, Microwave, Infrared, Visible Light (ROYGBIV), UV, X-Ray, Gamma
Whatās the different between a red and blue wavelength?
Red: shorter wavelength
Blue: long wavelength
Atomic Spectrum
When light from a heated element passes through a prism, it separates into distinct lines of color separated by dark areas that are called an atomic emission spectrum
What is the use of an atomic spectrum?
Each element has its own distinct emission spectrum
Helps with identification
What are the lines in an atomic spectrum associated with?
The changes in the energies of the electrons
Energy level
The specific energy of an electron in an atom
How are energy levels labeled?
They are assigned a principal quantum number represented with the letter n.
n = 1, n = 2ā¦
What happens when you add light energy to an atom?
First, the atoms is at its ground state. Once energy is added, the atom absorbs it and get excited and jumps to a further energy level(the more energy, the farther the energy level). However, the atom doesnāt like this unstable state and returns to its original ground state.
When the atom returns to its ground state, energy is released back in light form. This energy emitted is equal to the difference between the two energy levels the atom traveled between.
Sublevels
The arrangement of electrons that determines the physical and chemical properties of an element
Where are sublevels located?
In energy levels
How can you determine the amount of sublevels within an energy level?
The # of sublevels is equal to the principal quantum number of that energy level
What are the 4 different sublevels in ascending order?
s<p<d<f
What would the sublevels in an n = 3 energy level be?
s, p, and d
Organize the following in order (largest to smallest)
Electrons
Energy levels
Sublevels
Orbitals
Energy levels, sublevels, orbitals, electrons
How many electrons fit in an orbital and how are they arranged?
2
one up and one down
How many orbitals does each sublevel have and how many electrons can the entire thing hold??
s ā 1 orbital = 2 electrons
p ā 3 orbitals = 6 electrons
d ā 5 orbitals = 10 electrons
f ā 7 orbitals = 14 electrons
Orbital
A three-dimensional volume in which electrons have the highest probability of being found
Location of an electron describe in terms of probability (electron cloud)
S orbitals
Shown as spheres
Increase in size as n increases
What would an s orbital be called?
1s or any number based on its n value
P orbitals
Two lobes; like a ballon tied in the middle
The three p orbitals are arranged perpendicular to each other along the x, y, and z axes around the nucleus
Each piece is along a different axis
What are the names of the p orbital parts? (in n = 2)
2px, 2py, 2pz
The extra letter represents the direction
D orbitals
Four of the five d orbitals consist of 4 lobes that are aligned along of between different axes.
The fifth consists of two lobes (like a p orbital) with a doughnut-shaped ring around its center
What are the names of the d orbital parts?
dxy, dyz, dxz, dxĀ²-yĀ², dzĀ²
The Pauli Expulsion Principal
Each orbital can hold a max of two electrons
Electrons in the same orbital repel each other
Electrons in the same orbital must have their magnetic spins cancel (they spin in opposite directions)
What are the rules of drawing orbital diagrams?
Fill the orbitals and energy level from lowest to highest energy level
Each orbital holds 2 electrons max
Fill orbitals within the same sublevel one at a time before pairing electrons
Orbital order
1s2s2p3s3p4s3d4p5s4d5p
No commas
Use of electron configuration
Indicate placement of electrons
Show how electrons fill energy levels and sublevels in order of increasing energy
What can you do with really long electron configurations?
Write an abbreviated version using a noble gas
Go up one row and down to the noble gas
Put that noble gas in brackets and write the rest of the electron configuration
ex. SODIUM = [Ne] 3sĀ¹
What must you do with Helium when doing electron configurations?
Move it next to Hydrogen
Valence Electrons
In the outermost shell and are responsible for the chemistry and reactions
Valence Electron Configurations
The group # of s and p blocks tell you the # of outermost electrons
8A = 8 valence electrons
Octet Rule
8 = stability
Sublevel sections of the periodic table
First two = s
Last 6 = p
Transition metals = d
Bottom two rows = f
Lewis Symbols
Display valence electrons
How to draw Lewis Symbols
Draw electrons as dots in pairs
Go around the entire 4 sides AND THEN start to pair
Trends in the periodic table
Atomic Size and Metallic Character decrease left to right
Ionization Energy increases left to right
Atomic Size and Metallic Character increase top to bottom
Ionization Energy decreases top to bottom
Atomic Size
Affected by the attraction between the protons in the nucleus and the electrons in the outermost energy level
More protons = stronger attraction that brings the electrons closer = smaller overall size
Basically the radius
Ionization Energy
Energy needed to loose electron
If more protons are present, it will be more difficult to kick out electrons
When the space between the protons and electrons expand, as it does going down, the electrons are easier to kick out
What does it mean to ionize?
Loose an electron
Metallic Character
Ability to loose electrons easily
Metals have more metallic character, so as you go down the metals, they want to loose their electrons
As you go further towards the halogens, they want to gain the electrons and bond
What does this mean?
The energy of an electron is quantized
Electrons can have only specific energy values
What increases as the n # increases
Why?
The energy
The electrons are further away from the nucleus meaning the positive protons cannot combat its energy