Ch 6 Section 4 Flashcards Preview

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Flashcards in Ch 6 Section 4 Deck (28):
1

This difference is reflected in the unique properties of

Metals

2

Metals are much better electrical conductors than even

Molten ionic compounds

3

The electrical conductivity if metals is due to the highly mobile

Valence electrons of the atoms in metals

4

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

Electron-pair bonds between neutral atoms

5

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

Ions that are held in place in crystal structures

6

Chemical bonding is different in metals than it is in

Ionic, molecular or covalent-network compounds

7

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

Electrons

8

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

Vacant

9

D block metals also possess many vacant

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

10

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

Roam freely throughout the entire metal

11

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

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

12

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

Packed together in a crystal lattice

13

Metallic bonding is the chemical bonding that results from the

Attraction between metal atoms and the surrounding sea of electrons

14

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

Electrical and thermal conductivity characteristic of all metals

15

Metals are both strong... Of light

Absorbers and reflectors

16

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

Wide range of light frequencies

17

This absorption of light results in the

Excitation of the metal atoms electrons. To higher energy levels

18

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

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

19

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

Appearance: luster of metal surfaces

20

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

Malleability and ductility

21

Malleability is the ability of a substance to be

Hammered or beaten into thin sheets

22

Ductility is the ability of a substance to be

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

23

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

All directions throughout the solid

24

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

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