Metallic Bonding

Which is the best metal to use in an alloy to increase its electrical conductivity? A. Al B. Cu C. Fe D. Sb

Which element is likely to be the best conductor of electricity? A. copper B. lithium C. iodine D. silicon

Which is most likely the result of millions of metal atoms crowding together so that molecular orbitals become combined? A. the loss of metallic properties B. the formation of bands in a crystal C. the loss of valence electrons to other atoms D. the formation of localized valence electrons

Which property is true for metals? A. localized electrons B. high electronegativity C. low ionization energies D. tightly held valence electrons

The diagram is a representation of the electron sea model. mc003-1.jpg Which statement best describes what is happening in this model? A. The electrons are floating to the top of the nuclei of metal atoms. B. The electrons are sinking down between the nuclei of metal atoms. C. The electrons are moving easily between the nuclei of metal atoms. D. The electrons are in fixed positions between the nuclei of metal atoms.

Which statement is true when a crystal is formed from many metal atoms? A. There are no bands being formed. B. There are many molecular orbitals. C. There are only unshared atomic orbitals. D. There are many electrons lost to other atoms.

Which is a characteristic of the electron sea model for metallic bonding? A. Molecular orbitals overlap to produce bands. B. Atomic nuclei are arranged in a regular pattern. C. Electrons are in localized positions in the orbitals. D. Atomic nuclei are arranged in an irregular pattern.

Which property is better explained by the band theory than by the sea of electrons model? A. ductility B. thermal conductivity C. luster D. electrical conductivity

Which statement best describes the basis of the band theory of metallic bonding? A. Molecular orbitals overlap to form atomic orbitals in which the valence electrons of the atoms travel. B. Molecular orbitals overlap to form atomic orbitals in which all electrons of the atoms travel. C. Atomic orbitals overlap to form molecular orbitals in which the valence electrons of the atoms travel. D. Atomic orbitals overlap to form molecular orbitals in which all electrons of the atoms travel.

Which reason best explains why metals are ductile instead of brittle? A. because they have rigid bonds B. because they have flexible bonds C. because they easily lose electrons D. because they easily gain electrons

Which property does a metal with a large number of free-flowing electrons most likely have? A. very hard B. very brittle C. poor conductivity D. good conductivity

Which characteristics of metal atoms help explain why valence electrons in a metal are delocalized? A. Metal atoms are large and have high electronegativities. B. Metal atoms are small and have low electronegativities. C. Metal atoms are large and have low electronegativities. D. Metal atoms are small and have high electronegativities.

Which combination of factors is most suitable for increasing the electrical conductivity of metals? A. more valence electrons and larger atomic radius B. fewer valence electrons and larger atomic radius C. more valence electrons and smaller atomic radius D. fewer valence electrons and smaller atomic radius

What is another name for the molecular orbital theory of bonding in metals? A. band theory B. ionic bond theory C. covalent bond theory D. electron bond theory

In a piece of metal, what holds the atoms together? A. the positive charges of the nuclei and the localized electrons around them B. the negative charges of the nuclei and the localized electrons around them C. the positive charges of the nuclei and the negative charges of delocalized electrons D. the negative charges of the nuclei and the positive charges of delocalized electrons

Which of the following metal atoms would have the highest conductivity? A. the atom with the smallest radius and the fewest valence electrons B. the atom with the smallest radius and the most valence electrons C. the atom with the largest radius and the fewest valence electrons D. the atom with the largest radius and the most valence electrons