Periodic trends

Presentation

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Chemistry

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10th - 12th Grade

•

Practice Problem

•

Medium

•

NGSS

HS-PS1-1, HS-PS1-2

Standards-aligned

Clelia Sandino

Used 14+ times

FREE Resource

9 Slides • 19 Questions

Periodic trends

HELLO HELLO!! LET'S PRACTICE!

Periodic Trends: Patterns along with the periodic table

Affected by energy levels (periods)

Affected by effective nuclear charge and electron shielding

- effective nuclear charge: caused by the increasing positive charge of the nucleus, which attracts electrons toward the nucleus.

Atomic radius

Distance between the nucleus and outermost orbital

Electron shielding:

Electrons in the outermost shell are repelled (shielded) by electrons in the inner shells. This repulsion counteracts the attraction caused by the positive nuclear charge
Look at what happens as you go down a group and as you go across a period from left to right

Ionization energy trend

Amount of energy needed to remove an electron
Larger atoms have a tendency to have lower ionization energy while smaller ones have bigger ionization energy.

Electronegativity

The ability of an atom in a chemical compound to attract electrons from another atom in the compound (strength of an atom)
Fluorine has highest electronegativity

Electron Affinity

The energy that occurs when an electron is acquired by a neutral atom Most atoms release energy when they acquire electrons (favored) Energy is released which causes negative values

Differences: Electronegativity and electron affinity

EN: Ability of atoms to attract electrons from other elements, Applied to a single atom
EA: Amount of energy liberated when a molecule or a neutral atom tends to acquire an electron from other elements, either an atom or molecule
EN: The maximum value is when the attracting force is high
EA: The maximum value is when the nuclear force is high

Multiple Choice

Which periodic group has the smallest atomic radius?

Alkali metals

Halogens

Noble Gases

Transition metals

Multiple Choice

As you move down the periodic table atoms get bigger. This is because ____________.

The atoms have more mass.

The atoms have more protons.

The atoms have more energy levels

The atoms have more nuetrons

Multiple Choice

As you move down the periodic table atoms get bigger. This is because ____________.

The atoms have more mass.

The atoms have more protons.

The atoms have more energy levels

The atoms have more nuetrons

Multiple Choice

A Bromine ion gains 1 electron, which of the following is the correct symbol for a Bromine ion?

Br^-1

Br⁺¹

Br⁺⁷

Br^-7

Multiple Choice

What is the ion formed from Sulfur?

S⁺²

S^-2

S⁺⁶

S^-6

Multiple Choice

How many electrons would a Calcium ion gain/lose?

lose 1

gain 1

lose 2

gain 2

Multiple Choice

How many electrons would a Nitrogen ion gain/lose?

lose 5

gain 5

lose 3

gain 3

Multiple Choice

Why do elements form bonds?

to get a charge

so they can make friends

to become stable by getting a full valence shell

to become stable by increasing their mass

Multiple Choice

Which types of elements from anions?

metals

nonmetals

metalloids

noble gases

Multiple Choice

Which types of elements from cations?

metals

nonmetals

metalloids

noble gases

Multiple Choice

What is a positive ion called?

anion

cation

isotope

covalent

Multiple Choice

What is a positive ion called?

anion

cation

isotope

covalent

Multiple Choice

Which of the period 3 elements has the largest electronegativity?

Multiple Choice

Which of the alkaline-earth metals has the smallest electronegativity

Multiple Choice

Of the halogens, which has the smallest electronegativity?

Multiple Choice

Which of the metalloids has the smallest atomic radius?

Multiple Choice

Of the halogens, which has the smallest radius?

Multiple Choice

Which element in Period 2 has the greatest atomic radius?

Multiple Choice

Which element in Period 2 has the greatest atomic radius?

Periodic trends

HELLO HELLO!! LET'S PRACTICE!

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