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Periodic Table A Period Stephanie Shao Abigail Richardson (Periodicity,…
Periodic Table
A Period
Stephanie Shao
Abigail Richardson
Periodicity
Atomic Radius
Decreases left to right across a period, increases going down a group
The size of an atom from the nucleus to the outermost orbital
Ionization Energy
Increases left to right across a period, decreases going down a group
The energy needed to remove one electron from a neutral atom
Electron Affinity
Increases left to right across a period , decreases going down a group
The energy change that occurs when an electron is acquired by a neutral atom
Electronegativity
Increases left to right across a period , decreases going down a group
The measure of the ability of an atom to attract electrons
The tendency of elements to have similar properties when arranged by their atomic number
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Quantum Numbers
Principle Quantum Number
Indicates the main energy level occupied by the electron
Represented by n
Angular Quantum Number
Indicates the shape of the orbital
0 is less than or equal to l which is less than or equal to n-1
Represented by l
Magnetic Quantum Number
Indicates orientation of an orbital around the nucleus
Represented by ml
-l is less than or equal to ml which is less than or equal to l
Spin Quantum Number
Two possible values which indicate the two fundamental spin states of an electron in an orbital
1/2
-1/2
Represented by ms
The quantum numbers of Fluorine are n=2, l=1, ml=0, ms=-1/2
Properties of Specific Elements
Atomic Mass
Element Name
Element Symbol (Ne for Neon)
Atomic Number
Number of Protons
Number of Electrons (if not an ion)
Groups and Periods
Groups
Halogens
Group 17
Make salts when reacting with metals, and form acids when bonded to hydrogen
Noble Gases
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Group 18
Odorless, colorless, generally unreactive gases
Akaline Earth Metals
Group 2
Shiny, silvery-white, and somewhat reactive metals
Coinage Metals
Group 11
Alkali Metals
Group 1
Shiny, soft, and highly reactive metals
Volatile Metals
Group 12
Icosagens
Group 13
Crystallogens
Group 14
Pnictogens
Group 15
Chalcogens
Group 16
Periods
Period 1
Do not follow the octet rule
1s orbital
Elements: H, and He
Period 2
2s and 2p orbitals
Elements: Li, Be, B, C, N, O, F, and Ne
Period 3
All occur in nature
All have at least one stable isotope
3s and 3p orbital
Elements: Na, Mg, Al, Si, P, S, Cl, and Ar
Period 4
The first period with transition metals
4s, 4p, and 3d orbitals
First period with d orbital
Elements: K, Ca, Sc, Ti, V, Cr, Mn, Fe, Co, Ni, Cu, Zn, Ga, Ge, As, Se, Br, and Kr
Period 5
5s, 5p, and 4d orbitals
Elements: Rb, Sr, Y, Zr, Nb, Mo, Tc, Ru, Rh, Pd, Ag, Cd, In, Sn, Sb, Te, I, and Xe
Period 6
First period with f orbital
6s, 6p, 5d, and 4f orbitals
Elements: Cs, Ba, La, Ce, Pr, Nd, Pm, Sm, Eu, Gd, Tb, Dy, Ho, Er, Tm, Yb, Lu, Hf, Ta, W, Re, Os, Ir, Pt, Au, Hg, Tl, Pb, Bi, Po, At, and Rn
Period 7
All are radioactive
7s, 7p, 6d, and 5f orbitals
Elements: Fr, Ra, Ac, Th, Pa, U, Np, Pu, Am, Cm, Bk, Cf, Es, Fm, Md, No, Lr, Rf, Db, Sg, Bh, Hs, Mt, Ds, Rg, Cn, Nh, Fl, Mc, Lv, Ts, and Og
Electron Configuration
Describe an element by the electrons in its shells
Full Electron Configuration
For Chlorine, the electron configuration is 1s^(2)2s^(2)2p^(6)3s^(2)3p^(5)
Noble Gas Electron Configuration
For Chlorine, the electron configuration is [Ne]3s^(2)3p^(5)
Properties of Multiple Elements
Metals
An element that is a good conductor of heat and electricity
Tend to be shiny, solid at room temperature, ductile, and malleable
Non-metals
An element that is a poor conductor of heat and electricity
Tend to be brittle
Can be gas, liquid, or solid at room temperature
Metalloids
An element that has some characteristics of metals and non-metals
Tend to be semi-conductors and solid at room temperature
Noble Gases
