Atomic Structure and Bonds

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Intro chemistry topics (bonds)

By Távara

hold up some fingers, how do we feel today?

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temp check!

energy levels

covalent bonds

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New​

Atoms and their composition from element to element.​

Elements in the Periodic table. ​

Recap

Objectives

Fill in the Blanks

What are the three subatomic particles that make up an atom?

​Here is a diagram:

which particles are in the center? which one is outside?​

everything is made of elements, elements are made of atoms​

Multiple Choice

Which one has a positive charge, a negative charge, and no charge?

• Proton - positive,

  neutron - negative,

  electron - no charge

• proton - no charge, neutron - negative, electron - positive

• proton - positive, neutron - no charge, electron - negative

• proton - negative, neutron - no charge, electron - positive

Electrons are negatively charged and are attracted towards positively charged protons. The more electrons an atom has the more negatively charged the atom and vice versa. Atoms that are negatively charged are attracted to positively charged atoms.

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Electrons

Periodic table​

The periodic table gives you information on the structure of the atom of each element. ​

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The atomic number is the amount of protons in a nucleus and usually the same amount of electrons.

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The atomic mass is found by counting how many protons and neutrons in the nucleus of​ the atom.

​How to read elements​

Multiple Choice

Element: Hydrogen (H)

Atomic number 1:

Atomic Mass: 1.01

How many protons does this element have?

• 1

• 2

• 0

• -1

Multiple Choice

Element: Oxygen (O)

Atomic Number: 8

Atomic Mass: 16.00

how many neutrons does this element have?

• 7

• 8

• 6

• 9

Multiple Choice

Element: Potassium (K)

Atomic number: 19

Atomic mass: 39

How many electrons does this element have?

• 17

• 18

• 20

• 19

One of the most commonly used diagrams ​shows the electrons in energy levels surrounding the atoms nucleus. ​

How do we visualize this?

when atoms bond it is because they are trying to complete they energy level that surround a nucleus, completing the energy levels makes the atom more stable.​

Here is the musical chair analogy​.

Covalent Bonds

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take a look at the table below at a condensed table.

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what trends do you see on the groups/ families? (columns)

what trends do you see in the periods? (rows)

Some elements need more electrons than others to complete their energy levels.

The electrons on the outer most electron are known as valence electrons​. these are the only electrons in the atomic structure that can participate in chemical bonds.

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These are known as valence electrons

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Fill in the Blanks

Hydrogen

Atomic Number: 1

Atomic Mass: 1.01

How many valence electrons are on its outer energy level?

Fill in the Blanks

Lithium

Atomic Number: 3

Atomic Mass: 6.94 (rounded to ~7)

How many valence electrons are on its outer energy level?

Fill in the Blanks

Fluorine

Atomic Number: 9

Atomic Mass: 19

How many valence electrons are on its outer energy level?

Fill in the Blanks

Neon

Atomic Number: 10

Atomic Mass: 20.18

How many valence electrons are on its outer energy level?

Fill in the Blanks

Calcium

Atomic Number: 20

Atomic Mass: 40.08

How many valence electrons are on its outer energy level?

As we discussed the electron feels an attraction to a proton. when it comes in close proximity to another atom it might also become attracted to its proton. That may cause the atoms to bond. The outer energy levels usually holds only about 8 electrons. once there are 8 electrons the next electron goes to the next level.

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Take a look at this Covalent bond

This is them before. Note how many electrons each element has before bonding?

oxygen atom and hydrogen atoms

how many electrons do the hydrogen atoms have?

the oxygen atoms? ​

once they've bonded

Draw

draw the arrows representing the covalent bonds that make a Methane atom

Draw

draw the arrows representing the covalent bonds that make a Carbon Dioxide atom

Intro to Chemistry topics: Ionic Bonds

​Some text here about the topic of discussion.

Atoms that gain or lose electrons. ​

Ions​

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Known as a Cation

(kat-ion), The atom that LOSES an electron

Positive Ion​

known as an Anion (ann-ion)The atom that GAINS an electron​

Negative Ion

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atom of chlorine and sodium

before bond

note the thicker arrow​

atoms attract

Electrons from Sodiums outer level get transferred to Chlorine​

The two ions now attract each other BUT are not bonded the same as covalent bonds.

after bond

Draw

draw the arrows identifying the electrons being transferred. then below each atom draw a plus or minus indicating what type of ion it has become.