1.12 Periodic Trends -reason behind the trend "lesson" questions

​1.12 Periodicity - reasons behind the trends - lesson questions

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The atomic radius ​ decreases from left to right across a ​ period. This is because the number of ​

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in the nucleus are increasing causing the nucleus to have a greater effective ​

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; at the same time the electrons are being added to the ​

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and therefore there ​

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allowing for the attraction between the nucleus and the electrons to ​

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resulting in a smaller atom.

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protons

nuclear charge

same energy level

increase

neutrons

electrons

different energy level

decrease

is no increase in electron shielding

is an increase in electron shielding

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The atomic radius ​ increases from top to bottom down a group. Even though the number of​

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in the nucleus is increasing causing the nucleus to have a greater nuclear ​ charge, the electrons are being added to ​

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causing a(n)

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thus the attraction between the nucleus and the outer electrons ​

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thus the size of the atom ​

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.

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protons

neutrons

electrons

successively higher energy levels

increase in electron sheieding

decreases

increases

no change 

decrdecrease in electron shielding 

same energy level

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The ioniziation energy ​increases as you move ​left to right across a period . The part of the atom that holds the electrons in place is the ​

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due to it being ​

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and the electrons being negatively charged. When moving across a period the electrons are being added to ​

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thus there is​ ​

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causing a greater attraction between the nucleus and the electrons resulting in ​

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from the atom.

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The ionization energy decreases as you go down a group on the periodic table. This is due to the fact that the valence electrons are being placed on ​

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which cause them to become ​

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the nucleus thus causing a decrease in the ​

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resulting in ​

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being required to remove an electron from an atom in the bottom of a group than an electron of an atom ​

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successively higher energy levels

the same energy 

further from

closer to

effective nuclear charge

less energy

more energy

in the top of a group.

in the bottom of a group

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The electronegativity of an element represents the ability of an atom ​​

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. The trend in electronegativity as you move from left to right across a period is that the electronegativity increases. This is due to the fact that the radius of the atom has ​ ​

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causing there to be ​​

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between the nucleus and the outer parts of the atom. As the distance between the nucleus and the outer part of the atom ​ ​decrease the ability for the nucleus to attract electrons ​

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​ resulting in a​

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to attract electrons

repel electrons

decreased

less distance

increases

more distance 

higher electronegativity

lower electronegativity

Multiple Choice

Which of the following elements has the most "shielding" electrons?

• Nitrogen
• Phosphorus
• Lithium

• Helium

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As you move from down a group on the Periodic Table...

The number of energy levels ​​

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.

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As you move from left to right across a period on the Periodic Table...

The number of energy levels ​​ ​

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.

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As you move from down a group on the Periodic Table...

The number of core electrons ​​

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.

Match

Match the trend with the correct definition

• The strength of attraction between an atom's nucleus and the electrons in that atom.

• The distance from the center of an atom and the furthest electron. This is a measure of an atom's size.

• The energy required to remove an electron from an atom.

• The likelihood that that an atom will participate in a chemical reaction

Electronegativity

Atomic Radius

Ionization Energy

Reactivity

• Electronegativity

• Atomic Radius

• Ionization Energy

• Reactivity