Metallic Bonds and Ionic Bonds Flashcards

1
Q

How do cations form?

A

They lose an electron

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2
Q

How do anions form?

A

They gain an electron

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3
Q

What groups are more likely to form what type of ion?

A

Metals are more likely to form cations and nonmetals are more likely to form anions

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4
Q

What is the octet rule?

A

The rule where an element won’t be stable until it has 8 valence electrons

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5
Q

What suffix do all monoatomic anions have?

A

-ide

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6
Q

What is an electrolyte?

A

A compound that conducts electricity when dissolved in water

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7
Q

What are two reasons ionic compounds have high melting points?

A

They are extremely strong and form crystal lattices

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8
Q

Why are ionic compounds brittle?

A

Ions of the same charge are pushed up against each other when putting pressure on the compound, which makes them repel and shatter

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9
Q

What are the properties of metals?

A

Conductive, malleable, ductile, lustrous, and solid at room temperature

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10
Q

What is the “sea of electrons” model?

A

The electrons of metal atoms moving around because of the loose grip held on them

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11
Q

Whare does it mean when it is said that electrons in metals are “delocalized”?

A

It means that valence electrons are held loosely in metal atoms, making the “sea of electrons”

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12
Q

Why are metals good conductors?

A

Because electricity is just energy going through electrons, and since they are delocalized it is really easy for that energy to run through the metal

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13
Q

Why are metals considered to be crystalline?

A

Because they are arranged orderly when bonded

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14
Q

What is an alloy?

A

2 or more bonded elements where at least one is a metal

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15
Q

Why are alloys important?

A

Because they have better properties than pure metals

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16
Q

What are three examples of an alloy?

A

Brass, bronze, and steel