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• The number of valence electrons. 

The number of atomic orbitals.

• Number of electron shells an element's atoms have, which affects their chemical properties and atomic size.

The number of orbitals equals n^2.

The number of orbitals equals n+2

The number of orbitals equals n-2

The number of orbitals equals n/2

Group 1A: 1 valence electron

• Group 2A: 2 valence electrons

• Group 3A: 3 valence electrons

• Group 4A: 4 valence electrons

• Group 5A: 5 valence electrons

• Group 6A: 6 valence electrons

• Group 7A: 7 valence electrons

• Group 8A: 8 valence electrons

Group 1A: 2 valence electron

• Group 2A: 4valence electrons

• Group 3A: 6 valence electrons

• Group 4A: 8 valence electrons

• Group 5A: 10 valence electrons

• Group 6A: 12 valence electrons

• Group 7A: 14 valence electrons

• Group 8A: 16 valence electrons

• Group 1A: 8 valence electron

• - Group 2A: 7 valence electrons

• - Group 3A: 6 valence electrons

• - Group 4A: 5 valence electrons

• - Group 5A: 4 valence electrons

• - Group 6A: 3 valence electrons

• - Group 7A: 2 valence electrons

• - Group 8A: 1 valence electrons

• Metals: Atoms with properties like shiny appearance, good conductors of heat and electricity, malleability, and ductility.

• Non-metals: Atoms lacking metallic properties, often brittle, poor conductors of heat and electricity.

• Metalloids: Atoms with properties between metals and non-metals, sometimes acting as semiconductors. Examples include silicon and boron.

• Metals: Atoms lacking metallic properties, often brittle, poor conductors of heat and electricity.

• Non-metals: Atoms with properties between metals and non-metals, sometimes acting as semiconductors. Examples include silicon and boron.

• Metalloids: Atoms with properties like shiny appearance, good conductors of heat and electricity, malleability, and ductility.

None

• Metals:

• - Dull appearance

• - Good conductors of heat and electricity

• - Malleable and ductile

• - High melting and boiling points

• Non-metals:

• - Shiny appearance

• - Poor conductors of heat and electricity

• - Brittle

• - Low melting and boiling points

• Metalloids:

• - Properties between metals and non-metals

• - Can have characteristics of both

• - Some are semiconductors

• Metals:

• - Shiny appearance

• - Good conductors of heat and electricity

• - Malleable and ductile

• Non-metals:

• - Dull appearance

• - Poor conductors of heat and electricity

• - Brittle

• - Low melting and boiling points

• - Some are semiconductors

• Metalloids:

• - Properties between metals and non-metals

• - Can have characteristics of both

• - High melting and boiling points

• Metals:

• - Shiny appearance

• - Good conductors of heat and electricity

• - Malleable and ductile

• - High melting and boiling points

• Non-metals:

• - Dull appearance

• - Poor conductors of heat and electricity

• - Brittle

• - Low melting and boiling points

• Metalloids:

• - Properties between metals and non-metals

• - Can have characteristics of both

• - Some are semiconductors

• - Shiny appearance, good conductor of heat and electricity, malleable, ductile, high melting and boiling points: Non-metal

• - Dull appearance, poor conductor of heat and electricity, brittle, low melting and boiling points: Metal

• - Properties between metals and non-metals, can have characteristics of both, some are semiconductors: Metalloid

• - Shiny appearance, good conductor of heat and electricity, malleable, ductile, high melting and boiling points: Metal

• - Dull appearance, poor conductor of heat and electricity, brittle, low melting and boiling points: Non-metal

• - Properties between metals and non-metals, can have characteristics of both, some are semiconductors: Metalloid

• - Shiny appearance, good conductor of heat and electricity, malleable, ductile, high melting and boiling points: Metalloid

• - Dull appearance, poor conductor of heat and electricity, brittle, low melting and boiling points: Non-metal

• - Properties between metals and non-metals, can have characteristics of both, some are semiconductors: Metal

• - Alkali Metals: Lithium (Li), Sodium (Na), Potassium (K), Rubidium (Rb), Cesium (Cs), Francium (Fr)

• - Alkaline Earth Metals: Beryllium (Be), Magnesium (Mg), Calcium (Ca), Strontium (Sr), Barium (Ba), Radium (Ra)

• - Transition Metals: Scandium (Sc), Titanium (Ti), Vanadium (V), Chromium (Cr), Manganese (Mn), Iron (Fe), Cobalt (Co), Nickel (Ni), Copper (Cu), Zinc (Zn), Yttrium (Y), Zirconium (Zr), Niobium (Nb), Molybdenum (Mo), Technetium (Tc), Ruthenium (Ru), Rhodium (Rh), Palladium (Pd), Silver (Ag), Cadmium (Cd), Hafnium (Hf), Tantalum (Ta), Tungsten (W), Rhenium (Re), Osmium (Os), Iridium (Ir), Platinum (Pt), Gold (Au), Mercury (Hg), Rutherfordium (Rf), Dubnium (Db), Seaborgium (Sg), Bohrium (Bh), Hassium (Hs), Meitnerium (Mt), Darmstadtium (Ds), Roentgenium (Rg), Copernicium (Cn), Nihonium (Nh), Flerovium (Fl), Moscovium (Mc), Livermorium (Lv), Tennessine (Ts), Oganesson (Og)

• - Halogens: Fluorine (F), Chlorine (Cl), Bromine (Br), Iodine (I), Astatine (At)

• - Noble Gases: Helium (He), Neon (Ne), Argon (Ar), Krypton (Kr), Xenon (Xe), Radon (Rn)

• - Alkali Metals: Lithium (Li), Sodium (Na), Chlorine (Cl), Potassium (K), Rubidium (Rb), Cesium (Cs), Francium (Fr)

• - Alkaline Earth Metals: Beryllium (Be), Magnesium (Mg), Calcium (Ca), Strontium (Sr), Barium (Ba), Radium (Ra)

• - Transition Metals: Scandium (Sc), Titanium (Ti), Vanadium (V), Chromium (Cr), Manganese (Mn), Iron (Fe), Cobalt (Co), Nickel (Ni), Copper (Cu), Zinc (Zn), Yttrium (Y), Zirconium (Zr), Niobium (Nb), Molybdenum (Mo), Technetium (Tc), Ruthenium (Ru), Rhodium (Rh), Palladium (Pd), Silver (Ag), Cadmium (Cd), Hafnium (Hf), Tantalum (Ta), Tungsten (W), Rhenium (Re), Osmium (Os), Iridium (Ir), Platinum (Pt), Gold (Au), Mercury (Hg), Rutherfordium (Rf), Dubnium (Db), Seaborgium (Sg), Bohrium (Bh), Hassium (Hs), Meitnerium (Mt), Darmstadtium (Ds), Roentgenium (Rg), Copernicium (Cn), Nihonium (Nh), Flerovium (Fl), Moscovium (Mc), Livermorium (Lv), Tennessine (Ts), Oganesson (Og)

• - Halogens: Fluorine (F), Chlorine (Cl), Bromine (Br), Iodine (I), Astatine (At)

• - Noble Gases: Helium (He), Neon (Ne), Argon (Ar), Krypton (Kr), Xenon (Xe), Radon (Rn)

• How much an atom repels electrons in a chemical bond.

• How much an atom attracts electrons in a chemical bond.

• How many atoms and electrons in a chemical bond.

• The trend of electronegativity increases from left to right across a period and decreases from top to bottom within a group on the periodic table.

• The trend of electronegativity decreases from left to right across a period and increases from top to bottom within a group on the periodic table.

• The trend of electronegativity increases from right to left across a period and decreases from bottom to top within a group on the periodic table.

• The trend of electronegativity decreases from right to left across a period and increases from bottom to top within a group on the periodic table.

• 1. Alkali Metals (Group 4a)

• 2. Alkaline Earth Metals (Group 2A)

• 3. Transition Metals

• 4. Group 3A to 7A

• 5. Noble Gases (Group 8A).

• 1. Alkali Metals (Group 8A)

• 2. Alkaline Earth Metals (Group 7A)

• 3. Transition Metals (Group 2A)

• 4. Group 3A to 7A

• 5. Noble Gases (Group 1A).

• 1. Alkali Metals (Group 1A)

• 2. Alkaline Earth Metals (Group 2A)

• 3. Transition Metals

• 4. Group 3A to 7A

• 5. Noble Gases (Group 8A).

The energy needed to add more electrons to an atom.

The energy needed to remove an electron from an atom.

The energy needed to remove all electrons from an atom.

• The trend of ionization energy increases across a period from left to right and decreases down a group from top to bottom on the periodic table.

• The trend of ionization energy decreases across a period from left to right and increases down a group from top to bottom on the periodic table.

• The trend of ionization energy increases across a period from right to left and decreases down a group from top to bottom on the periodic table.

• 3. Alkali Metals (Group 1A)

• 4. Group 2A

• 5. Group 3A to 7A

• 1.Halogens (Group 7A)

• 2. Noble Gases (Group 8A)

• 1. Alkali Metals (Group 1A)

• 2. Group 2A

• 3. Group 3A to 7A

• 4. Halogens (Group 7A)

• 5. Noble Gases (Group 8A)

The distance from the center of a circle or sphere to its outer edge.

It refers to the time it takes for the atoms from the nucleus to get to the outermost electron shell.

The distance from the nucleus to the outermost electron shell.

• The trend of atomic radius decreases down a group and decreases across a period on the periodic table.

• The trend of atomic radius increases down a group and decreases across a period on the periodic table.

• The trend of atomic radius decreases down a group and increases across a period on the periodic table.

• The trend of atomic radius increases down a group and increases across a period on the periodic table.

• 1. Group 1A (Alkali Metals)

• 2. Group 7A (Halogens)

• 3. Group 8A (Noble Gases)

• 4. Group 2A

• 5. Group 3A to 7A

• 1. Group 2A

• 2. Group 7A (Halogens)

• 3. Group 1A (Alkali Metals)

• 4. Group 8A (Noble Gases)

• 5. Group 3A to 7A

• 1. Group 8A (Noble Gases)

• 2. Group 7A (Halogens)

• 3. Group 1A (Alkali Metals)

• 4. Group 2A

• 5. Group 3A to 7A

• How likely a substance is to undergo a chemical reaction with other substances.

Rearrangement of the atoms or molecules of two or more substances that come into contact with each other, resulting in the formation of one or more new substances.

Where a nuclear reaction is controlled, making it possible to create energy or any number of artificial elements.

• Reactivity tends to increase as you go down, and across a period, it tends to decrease from left to right.

• Reactivity tends to decreases as you go down, and across a period, it tends to increases from left to right.

• Reactivity tends to increase as you go down, and across a period, it tends to decrease from right to left.