Chemistry Bonding Test Review

What do the dots represent in electron dot structures?

• Total number of electrons in the atom

• Number of total Valence electrons in the atom

• Number of valence electrons in the cation that forms

• Number of valence electrons in the anion that forms

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NGSS.HS-PS1-1

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What happens in covalent bonds?

• Electrons are transferred from cations to anions

• Electrons are transferred from anions to cations

• Electrons are shared in the inner electron layers

• Valence electrons are shared between two atoms

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NGSS.HS-PS1-1

Ionic bonds form between ________ and _________

• two cations

• two anions

• one cation and one anion

• one atom and one ion

Which molecule has a pyramid shape?

• Water (H₂O)

• Ammonia (NH₃)

• Methane (CH₄)

• Carbon dioxide (CO₂)

How many valence electrons does the electron structure for bromide ion (Br-1) have?

• 0

• 1

• 7

• 8

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NGSS.HS-PS1-1

What are the valence electrons of an atom?

• The electrons that an atom gains when it becomes an anion

• The electrons that remain closest to the nucleus

• The electrons in the highest occupied energy level

• The electrons that an atom loses when it becomes a cation

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NGSS.HS-PS1-1

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How many electrons are shared in a double bond?

• 4

• 2

• 8

• 6

1.    ________According to Valence Shell Electron Pair Repulsion (VSEPR) theory, which statement is correct?

• If a molecule is bent, it will always have unpaired electrons around the central atom.

• If a molecule is made up of three atoms, it will always have a linear structure.

• If a molecule has four pairs of electrons, it will always have a tetrahedral structure.

• If a molecule has three atoms around a central atom, it will always be trigonal planar.

1.    Why do atoms form ionic and covalent bonds?

• to attain a noble-gas electron configuration

• to increase their atomic numbers

• to become ions to attract each other

• to become more polar

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NGSS.HS-PS1-1

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In Ammonia (NH₃) the central atom has one unshaired electron pair. How do the unshaired electrons affect the bond angle?

• They push the bonding pairs closer together, making the bond angle smaller.

• They pull the bonding pairs farther apart, making the bond angle larger.

• They have no effect on the bonding pairs; the bond angle is the same as it would be without them.

• They both push and pull the bonding pairs, making the bond angle increase and decrease in a cyclic pattern.