Periodic Table Trends and Compounds Study Guide Unit 2 Flashcards
Alkali Metals
Group 1A (Li, Na, K, Rb, Cs, Fr) except hydrogen
Alkaline Earth Metals
Group 2A (Be, Mg, Ca, Sr, Ba, Ra)
Halogen
Group 7A highly Reactive
Noble Gases
Group 8A Highly Unreactive Group
Transition Metals
Group B (in the middle)
Inner Transition Metals
Group B
ionization energy
The energy required to make an ion by removing an electron
Cation
Atom or group of atoms that has a positive charge
Anion
Atom or group of atoms that has a negative charge
Electronegativity
The tendency of atoms of the element to attract electrons
Molecule
Combination of a nonmetal and nonmetal NEED PREFIX
Formula Unit
Combination of a metal and nonmetal NO PREFIX
Ionic Compound
A force that holds oppositely charged particles together
Covalent Bond
The bond formed when two nonmetal atoms share electrons
Polyatomic Ion
Group of Atoms that have a positive and negative charge
octet rule
Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas usually eight valence electrons
Atomic size TRENDS
- Periodic Trend from LEFT to RIGHT down electrons are the same distance but are closer to the nuclei
- Group Trend going Down because outer electrons are in further energy levels
- The radius is C=0.77 A
Ionic Size TRENDS
- Decreases in size from left to right for both cations and anions (periodic)
- Group trend-increases in size going down
When do cations form
when an atom loses electrons
When do anions form
when an atom gains electrons
Factors of Ionizing Energy
- number of electrons (further the valence electrons are easier to pull off the electron)
- Shielding Effect (inner electrons decrease the effective nuclear charge)
- Size of the Nucleus ( the bigger the stronger the pull)
Ionizing Energy TRENDS
- Periodic- increases from left to right, electrons are the same distance but are pulled tighter by bigger nuclei
- Group- decreases from top to bottom because electrons are farther away and are shield by inner electrons
Electronegativity Trends
- Periodic- increases from right to left
2. Group- decreases going down
Where are Alkali Metals and What are they
ALL the way on the Left (Li, Na, K, Rb, Cs, Fr) DO NOT INCLUDE Hydrogen
Where are Alkaline Earth Metals and What are they
The column next to the Alkali Metals ( Be, Mg, Ca, Sr, Ba, Ra)
Where are Halogens and What are they
5th row in the known metals (F, Cl, Br, I, At)
Where are Noble gases and What are they
The last row in the periodic table (He, Ne, Ar, Kr, Xe, Rn) Don’t combine with any other elements
Examples of Metals
Any Alkali metal, Alkaline Earth metal, or Transition metal
Properties of Metals
- High Electrical Conductivity
- Shiny
- Ductile
- Malleable
Metalloids
Are on the stair line
B, Si, Ge, As, Sb, Te, Po
Properties of Metalloids
Properties of Metals and Non-Metals
- shiny or no
- ductile
- can or cannot conduct electricity
Properties of Non-Metals
- Not Shiny
- Don’t conduct electricity
- Many are in GAS form
Compare and Contrast Group A and Group B
Group A- Alkali Metals, Alkaline Earth Metals, Halogens, and Noble Gases
Group B- Transition Metals and Inner Transition Metals
Examples of Alloy
any metal
Compare and Contrast between Metallic, Covalent, and Ionic Bonds
Metallic bond hold METALS
Covalent bonds hold TWO NON-METALS
Ionic bonds held by negative or positive atoms or groups
Molecule v Formula Unit
Molecule: Non-Metals CO2 NEED PREFIXES Carbon Dioxide
Formula Unit- A metal and Non-Metal NO Prefixes
Formulas for the seven Diatomic Elements
Hydrogen- H2 Oxygen- O2 Nitrogen- N2 Chloride- Cl2 Bromine- Br2 Iodine- I2 Fluoride- F2
Formulas for Acids
ALWAYS H+
State- Aqueous (aq)
An Anion
An Alloy
Two metals
Charges on Alkali Metals, Alkaline Earth Metals, and Halogens
Alkali- +1
Alkaline- +2
Halogens- 3-
