mse 2001: test two study guide

Which of these elements would you expect to have the smallest electronegativity? Barium Strontium Sodium Chlorine Fluorine

Barium

The space group Cmmm has what lattice type? Body-centered Base-centered Face Centered Primitive No lattice type

Base-centered

The space group I4mm is of what lattice type? Base centered Symmetric Body centered Primitive Face centered

Body centered

True or False: Most man-made crystalline materials are single crystals, not polycrystalline. True False

False

Which bond will have the larger bond strength: Na-Cl or Mg-O? Na-Cl Mg-O

Mg-O

Will there be any difference in the ionic bonding energy for any of the atomic orientations shown above? No, all of these orientations with have the same bonding energy. Yes, at least one of these orientations will have a different bonding energy

No, all of these orientations with have the same bonding energy.

Will there be any difference in the metallic bonding energy for any of the atomic orientations shown above? Yes, at least one of these orientations will have a different bonding energy. No, all of these orientations with have the same bonding energy.

No, all of these orientations with have the same bonding energy.

True/False: One-fold (1-fold) rotational symmetry is permitted in crystal structures. True False

True

Predict which of these is the most likely oxidation state and electronic configuration for a ruthenium cation: 2+ oxidation state, [Kr] 5s04d5 1+ oxidation state, [Kr]5s24d5 3+ oxidation state, [Kr] 5s04d5 3+ oxidation state, [Kr] 5s24d6 8+ oxidation state, [Kr]5s04d0

3+ oxidation state, [Kr] 5s04d5

In a cubic unit cell, which of the following x-ray diffraction peaks will have the largest Bragg diffraction angle (2theta)? 301 221 003 220 111

301

In what order do the following orbitals fill? 3s, 4s, 3d, 4d, 4f, 5s 3s, 3d, 4s, 4d, 5s, 4f 3s, 4s, 3d, 5s, 4d, 4f 3s, 4s, 3d, 4d, 5s, 4f 3s, 3d, 4s, 4d, 4f, 5s

3s, 4s, 3d, 5s, 4d, 4f

Above is a picture of a face-centered cubic lattice. How many lattice points are in this unit cell? 1 4 8 7

4

Predict the most likely oxidation state for a titanium cation and which electrons will be lost to form that ion. I really should have watched Dr. Losego's videos. 4+ oxidation state, lose the 4s2 and the 4p2 electrons. 4+ oxidation state, lose the 4s2 and the 3d2 electrons. 2+ oxidation state, lose the 3d2 electrons. 2+ oxidation state, lose the 4s2 electrons.

4+ oxidation state, lose the 4s2 and the 3d2 electrons.

What is the outer most electronic orbital (valence shell) for strontium? 5p 6s 4p 4s 5s

5s

Yttrium's electronic configuration is [Kr]5s24d1. Which orbital is the valence orbital in elemental metallic yttrium? (This is the orbital that will do the metallic bonding.) None of these. 5s 4d 5s 5p

5s

If a tetragonal unit cell has "a" lattice parameters of 5 angstroms in length and a "c" lattice parameter of 2 angstroms in length, then the unit cell volume would be: 2x10-7 cm3 5x10-23 cm3 2x10-22 cm3 5x10-22 cm3 2x10-23 cm3 5x10-7 cm3

5x10-23 cm3

Barium is best classified as: An alkaline earth element A rare earth element. A transition metal A noble gas A alkali metal

An alkaline earth element

Consider the close-packed structures we have been discussing. What would be the coordination number for a single atom inside of a 3-dimensional close packed structure? Note: The coordination number is the number of atoms bonded to a given atom or in the case of close-packed metals the number of atoms "touching" a given atom. (These atoms can be considered "coordinated" to that atom.) This coordination number will be the same for every atom in the structure and will be the same irrespective of the stacking sequence (i.e., the same for HCP and FCC). Atoms are coordinated to 16 other atoms. Atoms are coordinated to 4 other atoms. Atoms are coordinated to 8 other atoms. Atoms are coordinated to 9 other atoms. Atoms are coordinated to 6 other atoms. Atoms are coordinated to 12 other atoms.

Atoms are coordinated to 12 other atoms.

The peaks observed in an x-ray diffraction experiment are the result of: Constructive interference from x-rays scattering from planes of atoms with a path length difference equal to half of the wavelength of the x-rays. Destructive interference from x-rays scattering from planes of atoms with a path length difference equal to half of the wavelength of the x-rays. Emission of x-rays due to the relaxation of core shell electrons in the material. Absorption of x-rays from excitation of core shell electrons in the material. Constructive interference from x-rays scattering from planes of atoms with a path length difference equal to the wavelength of the x-rays. Destructive interference from x-rays scattering from planes of atoms with a path length difference equal to the wavelength of the x-rays.

Constructive interference from x-rays scattering from planes of atoms with a path length difference equal to the wavelength of the x-rays.

Which of these planes is NOT in the {100} family for a tetragonal crystal? (A tetragonal unit cell drawn to proportion is included below for reference.) (A) (010) (B) (001) (C) (110) (D) Both B & C

(D) Both B & C

A series of similar metal alloys have the following enthalpies of fusion:Alloy A: 4 kJ / molAlloy B: 14 kJ / molAlloy C: 7 kJ/ molAlloy D: 20 kJ / molBased on this information, can you predictively rank these alloys from least stiff to most stiff? (Least Stiff) A < C < B < D (Most Stiff) (Least Stiff) A < B < C < D (Most Stiff) (Least Stiff) D < B < C < A (Most Stiff) It is NOT possible to make a reasonable prediction from the information provided.

(Least Stiff) A < C < B < D (Most Stiff)

Covalent bonds... ...are non-directional because they share electrons. ...are directional because they share electrons. ...are non-directional because they require the overlap of spherical orbitals. ...are directional because they require the overlap of non-spherical valence orbitals.

...are directional because they require the overlap of non-spherical valence orbitals.

Electronegativities... ...do not change from left to right across a period. ....are highest in the middle of a period of elements. ....decrease from left to right across a period. ...increase from left to right across a period.

...increase from left to right across a period.

The wavelengths of x-rays are similar in size to... ...the spacing between crystal planes in a material. ...the wavelength of IR radiation. ...grains in polycrystalline materials. ...the width of a human hair. ...an electron.

...the spacing between crystal planes in a material.

For a tetragonal unit cell with lattice parameters:a, b = 4 angstroms c = 6 angstroms. Which of the following x-ray diffraction reflections will occur at the SMALLEST Bragg diffraction angle? A. 100 B. 001 C. 010 Both A & B will have equivalently small diffraction angles. Cannot be determined from the given information.

001

For a cubic unit cell, how many planes are in the {110} family? 4 24 9 6 3 18 8 12

12

What is the electronic configuration for elemental Ti? 1s22s22p63s23p63d2 1s22s22p63s23p64s23d2 1s22s22p63s23p64s24d2 1s22s22p63d2 1s22s22p63s23p63d4

1s22s22p63s23p64s23d2

How many lattice points are in a body-centered tetragonal unit cell? 1 2 3 4 Not enough information is provided to determine.

2

If a lattice point is positioned on the "face" of a unit cell, amongst how many different unit cells is that lattice point shared? 1 unit cell 8 unit cells 2 unit cells 3 unit cells 4 unit cells

2 unit cells

Tellurides are interesting semiconducting materials that are useful for photovoltaics. What effective charge would you expect tellurium to adopt when it bonds to a metal to form a "metal telluride"? 2+ 1+ 1- 2- 3+ 3-

2-

Consider the atoms on the surface of a piece of metal that has an HCP crystal structure. Assuming the surface atoms are part of a close-packed plane, what would be the coordination number for one of these atoms? 6-fold coordinated 8-fold coordinated 9-fold coordinated 12-fold coordinated

9-fold coordinated

Iridium is best classified as: A transition metal An alkaline earth element A noble gas A halogen A rare earth element.

A transition metal

What types of orbitals exist in the n = 3 electronic shell of an atom? A. s-type orbitals B. p-type orbitals C. d-type orbitals D. f-type orbitals A. s-type orbitals only B. p-type orbitals only C. d-type orbitals only D. f-type orbitals only Both A & B (s- and p-type orbitals) A, B, and C (s-, p-, and d-type orbitals) A, B, C, and D (s-, p-, d-, and f-type orbitals)

A, B, and C (s-, p-, and d-type orbitals)

Metallic bonds... A. ...allow for high electrical conductivity in a material. B. ...are non-directional. C. ...allow a material to plastically deform. Both A & B Both A & C Both B & C All of the above (A, B, & C)

All of the above (A, B, & C)

Considering the ionic nature of the Mg-O and Na-Cl bonds, which of the following statements do you agree with? A. Mg-O likely forms a stronger bond than Na-Cl because it is made between divalent ions rather than monovalent ions. B. Mg-O is likely a double bond while Na-Cl is likely a single bond. C. Assuming bond distances are about equal, Mg-O will likely form a 4x stronger bond than Na-Cl. Both A & B are likely true. Both A & C are likely true. Both B & C are likely true. All are likely true.

Both A & C are likely true.

In the bond energy equation:Etotal = -A/x + B/x12 A. -A/x describes the energy of attraction between the two atoms forming the bond B. -A/x describes the energy of repulsion between the two atoms forming the bond C. B/x12 describes the energy of attraction between the two atoms forming the bond D. B/x12 describes the energy of repulsion between the two atoms forming the bond Both B & C are true. Both A & D are true.

Both A & D are true.

Which type(s) of bonding would you expect in the plastic material high-density polyethylene? (Choose the BEST answer.) Van der Waals bonding only Both ionic and van der Waals bonding. Ionic bonding only. Metallic bonding only Both covalent and van der Waals bonding. Covalent bonding only

Both covalent and van der Waals bonding.

If a crystal structure is found to have all of its lattice parameters equal to one another (a = b = c), which crystal class might it belong to? A. Cubic B. Tetragonal C. Hexagonal D. Rhombohedral Either A or B Either A or C Either A or D

Either A or D

The volume of an atom is mostly composed of Empty space Electrons Neutrons Protons The nucleus

Empty space

(True/False) In close-packing in 3D, the second row of atoms has only 4 interstices available True False

False

(True/False) The following notation is used to describe a family of planes: < h k l > True False

False

If Laue diffraction is performed on two different cubic crystal materials with the same space group, the crystal with the smaller lattice parameter will have the closer arrangement of diffraction spots. True False

False

Which of these statements about structures and close-packing sequences is true? Hexagonal close-packed (HCP) crystals have close-packed planes that stack in an ABABAB... pattern in terms of their relative orientation, while face-centered cubic (FCC) crystals have close-packed planes that stack in an ABCABC... pattern in terms of their relative orientation. Hexagonal close-packed (HCP) crystals have close-packed planes that stack in an ABABAB... pattern in terms of their relative orientation, while face-centered cubic (FCC) crystals have close-packed planes that stack in an ABBABBA... pattern in terms of their relative orientation. Hexagonal close-packed (HCP) crystals have close-packed planes that stack in an ABCABC... pattern in terms of their relative orientation, while face-centered cubic (FCC) crystals have close-packed planes that stack in an ABABAB... pattern in terms of their relative orientation. Hexagonal close-packed (HCP) crystals have close-packed planes that stack in an ABBABBA... pattern in terms of their relative orientation, while face-centered cubic (FCC) crystals have close-packed planes that stack in an ABCABC... pattern in terms of their relative orientation. Hexagonal close-packed (HCP) crystals have close-packed planes that stack in an ABBABBA... pattern in terms of their relative orientation, while face-centered cubic (FCC) crystals have close-packed planes that stack in an ABABAB... pattern in terms of their relative orientation.

Hexagonal close-packed (HCP) crystals have close-packed planes that stack in an ABABAB... pattern in terms of their relative orientation, while face-centered cubic (FCC) crystals have close-packed planes that stack in an ABCABC... pattern in terms of their relative orientation.

A body-centered lattice is denoted by the abbreviation: F B V A C I

I

The space group P622 has (1) what type of lattice and (2) what type of point group symmetry? It is a primitive lattice and has the 622 type of point group symmetry. It is a primitive lattice and has a hexagonal type of point group symmetry. It is a primitive lattice and has the 622 type of point group symmetry. It is a body-centered lattice and has a hexagonal type of point group symmetry. It is a face-centered cubic lattice and has a hexagonal type of point group symmetry.

It is a primitive lattice and has the 622 type of point group symmetry.

Based solely on their electronic configurations, which of these metals would you expect to have the largest saturation magnetization? (Assume no electrons are transferred between orbitals.) Manganese Iron Vanadium Zinc Palladium

Manganese

The intermetallic Al3Ni will PRIMARILY exhibit what type of bonding? "James Bond"ing Ionic van der Waals Hydrogen Covalent Metallic

Metallic

Which type of bonding listed below would best support high electrical conductivity in a material? Covalent Bonding Ionic Bonding Metallic Bonding Van der Waals Bonding

Metallic Bonding

Which of these elements would you expect to have the highest electronegativity? Barium Oxygen Phosphorous Molybdenum

Oxygen

The numbers and hands on this wristwatch will continue to "glow green" for an hour or more without any further stimulation. This is an example of what phenomenon? Fluorescence Phosphorescence Glowourescence Phosphorescence Emittance Optical Absorption

Phosphorescence

When integrating from infinity to some finite distance, what should the sign be of the potential energy (U) in this portion of the force-bond curve? Negative (-) Potential Energy Positive (+) Potential Energy

Positive (+) Potential Energy

Which Bravais lattice type is shown here? (Note that all sides of this unit cell have the same length and all interaxial angles are the same.) Primitive Hexagonal Primitive Monoclinic Base-centered Orthorhombic Primitive Orthorhombic Primitive Rhombohedral

Primitive Rhombohedral

This crystal class has lattice parameters that are all the same and interaxial angles that are all the same but are NOT 90°. Orthorhombic Cubic Triclinic Rhombohedral Tetragonal

Rhombohedral

What does it mean if a crystal structure has 3-fold rotational symmetry? The crystal structure will look the same before and after a rotation of 3° around this axis of symmetry. The crystal structure will look the same before and after rotating it 3 times in any direction. Three different axes of symmetry rotation are available to replicate the structure. The crystal structure will look the same before and after rotating it 60° around this axis of symmetry. The crystal structure will look the same before and after a rotation of 120° around this axis of symmetry.

The crystal structure will look the same before and after a rotation of 120° around this axis of symmetry.

Cobalt can have either an FCC or HCP structure. At room temperature, how would you expect the mass densities of the FCC and HCP forms of cobalt to compare? The density of FCC cobalt will be GREATER THAN the density of HCP cobalt. The density of FCC cobalt will be LESS THAN the density of HCP cobalt. The density of FCC cobalt will be EQUAL TO the density of HCP cobalt. It is impossible to determine with the information given.

The density of FCC cobalt will be EQUAL TO the density of HCP cobalt.

Below are two plastic cups both made out of the polymer, (C8H8)n. Which do you expect to be less dense and why? (one is styrofoam and the other is a plastic cup) The styrofoam cup is likely less dense because making the polymer into a foam adds more porosity to the material. The polystyrene cup is likely less dense because it is made of lower atomic number elements. The styrofoam is likely less dense because it is made of lower atomic number elements. The cups likely have the same density because they are made out of the exact same polymer. The polystyrene cup is likely less dense because it has more porosity than the styrofoam cup.

The styrofoam cup is likely less dense because making the polymer into a foam adds more porosity to the material.

(True/False) As you compare atoms of increasing atomic number, the atomic mass tends to increase at a higher rate than the atomic volume. True False

True

(True/False) Grain boundaries are the boundaries where a series of mis-oriented single crystals meet True False

True

(True/False) X-ray diffraction can be used to determine the atomic spacing between crystalline planes in a solid. True False

True

Will there be any difference in the covalent bonding energy for any of the atomic orientations shown above? No, all of these orientations with have the same bonding energy. Yes, at least one of these orientations will have a different bonding energy.

Yes, at least one of these orientations will have a different bonding energy.

What is the expected electronic configuration of elemental (non-ionized) copper? [Ar] 4s13d10 [Kr] 4s13d10 [K] 4s23d9 [Ar] 4s23d9

[Ar] 4s13d10

What is the electronic configuration for elemental Ti? [Ar]3d4 [Kr]4s23d2 [Ar]3d2 [Kr]3d2 [Ar]4s23d2

[Ar]4s23d2

A material will have a high elastic modulus if its Energy-Bond Distance curve exhibits: a large radius of curvature and a small second derivative at the global minimum of the plot. a small radius of curvature and a small second derivative at the global minimum of the plot. a large radius of curvature and a large second derivative at the global minimum of the plot. a small radius of curvature and a large second derivative at the global minimum of the plot.

a small radius of curvature and a large second derivative at the global minimum of the plot.

A metal with a face centered cubic crystal structure is composed of... non-close-packed planes with a repeating stacking sequence of ABCABC... close-packed planes with 6-fold rotational symmetry that repeat in a stacking sequence of ABCABC... close-packed planes with 6-fold rotational symmetry that repeat in a stacking sequence of ABAB... close-packed planes with 4-fold rotational symmetry that repeat in a stacking sequence of ABCABC... close-packed planes with 4-fold rotational symmetry that repeat in a stacking sequence of ABAB... non-close-packed planes with a repeating stacking sequence of ABAB...

close-packed planes with 6-fold rotational symmetry that repeat in a stacking sequence of ABCABC...

Positively charged ions are called anions. true false

false

The bonds between Fe-Fe in a steel alloy are primarily considered to be covalent. true false

false

Van der Waals bonding is so weak that it serves no purpose in engineering design. true false

false

To which crystal class does the space group I4mm belong? tetragonal orthorhombic monoclinic cubic hexagonal rhombohedral

tetragonal

To which point group does the space group I4mm belong? 4 I4 4mm mm tetragonal 4mm cubic

tetragonal

Because of their rigid bonding angles, covalent solids usually have more open crystal structures than ionic solids. true false

true

How do you notate this family of planes in a cubic lattice using Miller indices notation? (100), (010), (001), (-100), (0-10), (00-1) {100} 100 [100] (100) <100>

{100}