Which of the following statements concerning molecular orbital (MO) bond theory is/are correct?
1. MO theory can describe molecular bonding in excited states. 2. Molecular orbitals are obtained from the combination of atomic orbitals. 3. MO theory predicts that electrons are delocalized over the molecule through molecular orbitals. A.) 1 only B.) 2 only C.) 3 only D.) 1 and 2 E.) 1, 2, and 3
Which statement about the formation of a boron trifluoride molecule, BF3, from one boron atom and.....?
... three fluorine atoms is not correct? a) During the hybridization event, an empty 2pz orbital is “carried along.” b) Three sp2 hybrid orbitals are created as a result of a hybridization event. c) The hybridization of the fluorine atoms occurs as a result of the use of promotion energy. d) The resultant geometry is trigonal planar, with observed bonding angles of exactly 120°.
Which statement is true?
E. None of the above as A. Particles of different masses have the different speed at a given temperature. B. The larger a molecule, the slower it will effuse. C. For a given gas, the lower the temp, the slower it will effuse. D At very high pressures, a gas will occupy a smaller volume than predicted by the ideal gas law.
Which of the following statements is TRUE?
With all due respect, no, the answer is not (d). a. Is false. Molecules at the same speed have the same average kinetic energy, but the speed varies inversely with the mass. b. Is true. At a high pressure, and the actual volumes of the molecules themselves result in an increase in the volume over that predicted by the ideal gas equation. Contrary to the kinetic molecular theory, real gas molecules do have finite volumes. c. Is false. If "larger" means "heavier" then it will effuse more slowly. The effusion rate is inversely proportional to the mass. d. Is false. The effusion rate is directly proportional to temperature. The higher the temperature, the faster the molecules are moving and the greater the effusion rate.
What are some examples of polar and non polar molecules?
Polar molecules occur when two atoms do not share electrons equally in a covalent bond.A dipole forms, with part of the molecule carrying a slight positive charge and the other part carrying a slight negative charge. This happens when there is a difference between the electronegativity of each atom. An extreme difference forms an ionic bond, while a lesser difference forms a polar covalent bond. Fortunately, you can look up electronegativity on a table to predict whether or not atoms are likely to form polar covalent bonds. If the electronegativity difference between the two atoms is between 0.5 and 2.0, the atoms form a polar covalent bond. If the electronegativity difference between the atoms is greater than 2.0, the bond is ionic. Ionic compounds are extremely polar molecules.Examples of polar molecules include:water - H2Oammonia - NH3sulfur dioxide - SO2hydrogen sulfide - H2Sethanol - C2H6ONONPOLAR MOLECULESWhen molecules share electrons equally in a covalent bond there is no net electrical charge across the molecule.In a nonpolar covalent bond, the electrons are evenly distributed. You can predict nonpolar molecules will form when atoms have the same or similar electronegativity. In general, if the electronegativity difference between two atoms is less than 0.5, the bond is considered nonpolar, even though the only truly nonpolar molecules are those formed with identical atoms.Examples of nonpolar molecules include:any of the noble gasses: He, Ne, Ar, Kr, Xe (These are atoms, not technically molecules.)any of the homonuclear diatomic elements: H2, N2, O2, Cl2 (These are truly nonpolar molecules.)carbon dioxide - CO2benzene - C6H6carbon tetrachloride - CCl4methane - CH4ethylene - C2H4hydrocarbon liquids, such as gasoline and toluenemost organic molecules
Can you help with with four Chemistry problems about Molecular Orbital Theory and Valence Bond Theory please?
1. Which statement about molecular orbital theory is not true? a. The delocalizing of electrons through orbital networking in molecules is explained by molecular orbital theory and accounts for many of the properties of metals. b.Molecular orbital theory explains how orbitals can span large ranges of atoms in a molecule. c.Molecular orbital theory sometimes helps explain the color of particular molecules. d. Molecular orbital theory leads to more accurate bond order values. 2. Which statement best explains the difference between the electron distributions of a bonding orbital (e.g., H2) and an anti-bonding orbital (e.g., He2)? a.Anti-bonding orbitals and bonding orbitals have similar distributions. The difference is in the overall electron density between atoms. b.In a bonding orbital situation, the electron distribution is between the nuclei, because both nuclei want to share the electrons. In an anti- bonding circumstance, the electron distribution is around each atom. There is a void between the nuclei and the nuclei repel each other. 3. Which statement about molecular orbital theory is not true? a.The delocalizing of electrons through orbital networking in molecules is explained by molecular orbital theory and accounts for many of the properties of metals. b.Molecular orbital theory explains how orbitals can span large ranges of atoms in a molecule. c.Molecular orbital theory sometimes helps explain the color of particular molecules. d.Molecular orbital theory leads to more accurate bond order values. 4. We learned that four new molecular orbitals are created from the p orbitals for each carbon atom in the butadiene molecule (the axes perpendicular to the page). Which statement about these molecular orbitals is NOT true? a. The four molecular p orbitals of the four carbon atoms can be lined up parallel in order to create four new molecular orbitals. b.The electrons in the new molecular orbitals benefit because they are not confined to just one atom. c.The electrons, because of the new molecular orbits, are spread out over the entire molecule. d. As a result of the new molecular orbitals, the bond between the second and third carbon atoms is not really a single bond. In fact, the bond should be shorter. Thank you for your help!
Which of the following is not true of molecular orbitals?
Which of the following is not true of molecular orbitals? a) The number of molecular orbitals formed is always equal to the number of atomic orbitals combined. b)A molecular orbital can accommodate up to two electrons. c)When electrons are added to orbitals of the same energy, the most stable arrangement is predicted by Hund's rule d)The number of electrons in molecular orbitals is equal to the sum of all the valence electrons on the bonding atoms.
How does the boron molecule B2 exist according to the molecular orbital theory (MOT) while it does not complete its octet rule?
B2 is a known molecule in gas phase, although not very stable, whose existence has been predicted in terms of MOT because it has a Bond Order greater than zero (in the case of B2, the bond order is 1).The covalent bond between the two B atoms is a single bond and the corresponding MOT calculations show agreement with this:BO = (1/2) x (electrons in bonding MOs - electrons in antibonding MOs).According to this simple rule, a B2 molecule is predicted to exist (which is true, BO = 1), an O2 molecule is predicted to exist and to be stable (true, BO = 2), and an N2 molecule is predicted to exist and to be very stable (true, BO = 3).On the other hand, a Be2 molecule is predicted not to exist (true, BO = 0).Ah, the B2 molecule does not complete its octet indeed. It is a paramagnetic diradical. If you cool down the temperature you turn on more stable interactions among adjacent B atoms that can overcome the (weak) B-B single bond and, eventually, account for the existence of elemental boron as a giant molecular structure.
Which of the Following is NOT true about OSMOSIS?
A. Its a Passive Process B.Water will move from an area where there is less "free water" molecules to an area where there are more "free waters" C.A simple way to predict the direction of water movement is to remember that water follows solute. D.When the water has reached equilibrium, water will continue to cross the membrane but there will be no NET change in concentration. E. All of these