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
Metallic bond strength varied with the nuclear charge of the
Metal atoms and the number of electrons in the metals electron sea
26
Both of these factors (factors of variation f metallic bond strength) are reflected in s metals
Enthralled if vaporization
27
The amount of energy required to vaporize the metal is a measure of the
Strength of the bonds that hold the metal together
28
The enthalpy of vaporization is defined as the amount of energy absorbed as
Heat when a specified amount of a substance vaporizes at constant pressure