2.2 Study Guide Flashcards

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1
Q

Which charges attract?

A

Different charges attract.

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2
Q

Which charges repel?

A

Similar charges repel.

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3
Q

Please give an example of which charges repel and which attract.

A
  • Electrons with electrons repel.
  • Protons and electrons attract.
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4
Q

What is the relationship between coulombic attraction and amount of charge?

A

Direct relationship. As either charge increases, the force will also increase by the same magnitude.

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5
Q

What is the relationship between coulombic attraction and distance?

A

Inverse relationship. As the distance between them increases, the force of attraction decreases.

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6
Q

Which atom has a higher electronegativity? Please explain. Hydrogen, argon, helium, or sodium.

A

Helium. This is because electronegativity increases as you move from left to right on the periodic table and decreases as you move down.

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7
Q

Which atom has a stronger or weaker attraction for valence electrons? Please explain. Fluorine or francium?

A
  • Stronger = Fluorine because it has a stronger pull and is closer to the nucleus. It attracts the most.
  • Weaker = Francium because it’s further away from the nucleus and attracts the lowest amount.
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8
Q

Electrons to electrons do what?

A

Repel.

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9
Q

Inverse relationship is the relationship between what?

A

The relationship between distance and coulombic attraction.

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10
Q

Protons to electrons do what?

A

Attract.

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11
Q

Direct relationship is the relationship between what?

A

The relationship between coulombic attraction and the amount of charge.

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12
Q

The attraction of the nucleus to valence electrons depends on?

A
  • The amount of protons (more protons + more charge = more coulombic attraction.)
  • Distance from the nucleus (more distance = less coulombic attraction + electrons in between shield/repel).
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