Covalent and Ionic Bond Practice

When two atoms share electrons, a chemical bond is formed.  This type of bond is called:

• covalent bond

• ionic bond

• crystal bond

• polyatomic bond

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NGSS.HS-PS1-1

How do covalent bonds form?

• Donating & receiving valence e- between atoms.

• Opposite slight charges attract each other between compounds.

• I don't know - I fell asleep in class.

• Sharing valence e- between atoms.

Is this image an example of covalent bonding?

• Yes

• No

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NGSS.HS-LS1-6

What can be generalized about covalent bonds?

• Electrons will be exchanged.

• Electrons will be transferred.

• Electrons will be given and taken.

• Electrons will be shared.

Ionic bonds are between ​ (a)   and ​ (b)   in these compounds electrons are ​ (c)   and ​ (d)   . Covalent bonds are between nonmetals ​ In these compounds electrons are ​ (e)  

• metals
• nonmetals
• gained
• lost
• shared

Tags

NGSS.HS-PS1-2

In ionic bonds, electrons are ​ (a)   rather than being shared. When writing ​ a Lewis dot structure for an ionic compound, the elements' symbols are shown in a ​ (b)   with their charge and the electrons that make the ion stable. In a covalent bond, the valence electrons are ​ (c)   . When writing a Lewis dot structure for a covalent compound, the elements' symbols are written down, and the ​ (d)   electrons surround each symbol. At least one ​ (e)   of electrons are shared between the two elements.

• transferred

• bracket

• shared

• valence

• pair

Match the following

• an atom with a negative charge

• Covalent bonds

• an atom with a positive charge

• Ion

• bond metals to non-metals

• Cation

• an atom with a charge

• Anion

• bond non-metals to non-metals

• Ionic bonds

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NGSS.HS-PS1-3

What is it called if there are three-pairs of electrons being shared?

• Triple bond

• Bond length

• Tribond

• Chocolate Mousse

What two types of atoms make a covalent bond?

• 2 Nonmetals

• 1 Nonmetal & 1 Metal

• 2 Metals

• 2 Noble Gases

How many electrons are shared in a double bond?

• 2

• 4

• 6

• 8