Ch 6 Section 4 Flashcards

1
Q

This difference is reflected in the unique properties of

A

Metals

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2
Q

Metals are much better electrical conductors than even

A

Molten ionic compounds

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3
Q

The electrical conductivity if metals is due to the highly mobile

A

Valence electrons of the atoms in metals

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4
Q

The mobility in metals valence electrons is not possible in molecular compounds in which electrons are localized I.

A

Electron-pair bonds between neutral atoms

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5
Q

The mobility in metals valence electrons is not possible in solid ionic compounds in which electrons are bound to individual

A

Ions that are held in place in crystal structures

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6
Q

Chemical bonding is different in metals than it is in

A

Ionic, molecular or covalent-network compounds

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7
Q

The highest energy levels of most metal atoms are occupied by very few

A

Electrons

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8
Q

In s-block metals one or two valence electrons occupy the outermost orbital and all three outermost p orbitals are

A

Vacant

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9
Q

D block metals also possess many vacant

A

D orbitals in the energy level just below their highest energy level

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10
Q

Within s metal the vacant orbitals in the atoms outer energy levels overlap allowing the outer electrons of the atoms to

A

Roam freely throughout the entire metal

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11
Q

The electrons are dr localized meaning that they do not belong to

A

Any one atom but move freely about the metals network of empty atomic orbitals

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12
Q

Mobile electrons form a sea of electrons around the metal atoms which are

A

Packed together in a crystal lattice

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13
Q

Metallic bonding is the chemical bonding that results from the

A

Attraction between metal atoms and the surrounding sea of electrons

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14
Q

The freedom of electrons to move in a network of metal atoms accounts for the high

A

Electrical and thermal conductivity characteristic of all metals

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15
Q

Metals are both strong… Of light

A

Absorbers and reflectors

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16
Q

Because they contain many orbitals separate by extremely small energy differences metals can absorb a

A

Wide range of light frequencies

17
Q

This absorption of light results in the

A

Excitation of the metal atoms electrons. To higher energy levels

18
Q

In metals the electrons immediately fall back down to lower levels emitting

A

Energy in the form of light at a frequency similar to the absorbed frequency

19
Q

Re-radiated (reflected) light is responsible for the metallic

A

Appearance: luster of metal surfaces

20
Q

Most metals are easy to form into desired shapes due to their

A

Malleability and ductility

21
Q

Malleability is the ability of a substance to be

A

Hammered or beaten into thin sheets

22
Q

Ductility is the ability of a substance to be

A

Drawn pulled or extruded through a small opening to produce a wire

23
Q

The malleability and ductility of metals are possible because metallic bonding is the same in

A

All directions throughout the solid

24
Q

When struck one plane of atoms in a metal can slide past another without encountering

A

Resistance or breaking bonds

25
Q

Metallic bond strength varied with the nuclear charge of the

A

Metal atoms and the number of electrons in the metals electron sea

26
Q

Both of these factors (factors of variation f metallic bond strength) are reflected in s metals

A

Enthralled if vaporization

27
Q

The amount of energy required to vaporize the metal is a measure of the

A

Strength of the bonds that hold the metal together

28
Q

The enthalpy of vaporization is defined as the amount of energy absorbed as

A

Heat when a specified amount of a substance vaporizes at constant pressure