Periodic Table Trends

Why are elements at the bottom of the PT larger than those at the top?

• They have more orbitals

• They have more valence electrons

• They have more charge

• They have a weaker attraction

Why are elements at the top of the PT have higher electronegativity than those at the bottom?

• They have fewer orbitals, this makes them smaller and since electrons are closer to the nucleus there will be a stronger ability to attract electrons

• They have fewer valence electrons

• They have more orbitals, this makes them larger and since electrons are further from the nucleus there will be a stronger ability to attract electrons

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Why are elements at the top of the PT have higher ionization energy than those at the bottom?

• They have fewer orbitals, this makes them smaller and since electrons are closer to the nucleus the attraction is stronger which makes it more difficult to remove

• They have fewer valence electrons

• They have more orbitals, this makes them larger and since electrons are further from the nucleus the attraction is weaker which make it easier to remove

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Why are elements at the left of the PT larger than those at right?

• They have fewer orbitals

• They have more valence electrons

• Their electrons have a stronger attraction because there's more charge

• Their electrons have a weaker attraction because there's less charge

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Why are elements at the right of the PT have more electronegativity than those at left?

• They have fewer orbitals

• They have more charge which gives them a stronger attraction for electrons. (Non-metals form anions)

• The have less valence electrons

• They have less charge which gives them a stronger attraction. (Metals form cations)

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Why are elements at the right of the PT have higher ionization energy than those at left?

• They have more orbitals

• Since they are much larger its difficult to find their valence electrons

• They have more charge and are closer to completing the octet rule which is difficult to remove electrons

• They have less charge and its very easy to remove electrons from metals

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What is the difference between ionization energy and electronegativity?

• Ionization energy is the ability to attract a valence electron while, electronegativity is the energy needed to remove a valence electron.

• Ionization energy is the energy needed to remove a valence electron while, electronegativity is the ability to attract a valence electron.

• Ionization energy is the level of attraction between electrons and the nucleus while, electronegativity is the sharing of pairs of electrons.

What is the difference between electronegativity and atomic radius?

• electronegativity is the level of attraction between electrons and the nucleus while, atomic radius is the energy needed to remove electrons.

• electronegativity is the energy needed to remove electrons while, atomic radius is the level of attraction between electrons and the nucleus.

• electronegativity is the level of attraction between electrons and the nucleus while, atomic radius is the size of the atom

Beryllium (Be) has an atomic number of 4 & Magnesium (Mg) has an atomic number of 12. They have very similar chemical properties and will behave the same in a chemical reaction. How should they be placed on the periodic table?

• They should be placed in the same group with Mg on the top and Be below.

• They should be placed in the same group with Be on the top and Mg below.

• They should be placed in the same period with Mg on the left and Be on the right.

• They should be placed in the same period with Be on the left and Mg right.

Which are most reactive families on the periodic table.

• Alkali metals & Transition Metals

• Noble gases & Oxygen Family

• Halogens & Alkali metals

• Halogens & Noble gases