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

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Science

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9th - 12th Grade

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Practice Problem

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Easy

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NGSS

HS-PS1-1, HS-PS1-2, HS-PS1-3

Standards-aligned

Tania Murphy

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1 Slide • 10 Questions

1.12 Periodicity - reasons behind the trends - lesson questions

Drag and Drop

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

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

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

and therefore there

allowing for the attraction between the nucleus and the electrons to

resulting in a smaller atom.

Drag these tiles and drop them in the correct blank above

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

Drag and Drop

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

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

causing a(n)

thus the attraction between the nucleus and the outer electrons

thus the size of the atom

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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

Dropdown

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

due to it being

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

thus there is

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

from the atom.

Drag and Drop

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

which cause them to become

the nucleus thus causing a decrease in the

resulting in

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

Drag and Drop

The electronegativity of an element represents the ability of an atom

. 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

causing there to be

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

resulting in a

Drag these tiles and drop them in the correct blank above

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

Dropdown

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

The number of energy levels

Dropdown

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

The number of energy levels

Dropdown

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

The number of core electrons

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

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