Answer:
B) There are weak interactions between the CO2 molecules.
Explanation:
Carbon dioxide is composed of one carbon atom that is structured between two atoms of oxygen, they are bonded with double bond and the CO2 is symmetrical because of the arrangement of the bond between them.It is less electronegative than Oxgen, this gives Oxgen the ability to attract the electron to themselves, and there is no intermolecular existing within carbon dioxide other bands waal forces.Compounds that are gases under the condition of room temperatures, and pressure usually have have small molecules. and their molecules is usually have van der Waals forces acting between them and theses forces are weak.This allows carbon dioxide molecules to be able to move freely as a gas.
molecule (hope this helps :))
Answer:
20.3 % NaCl
Explanation:
Given data:
Mass of solute = 45.09 g
Mass of solvent = 174.9 g
Mass percent of solution = ?
Solution:
Mass of solution = 45.09 g + 174.9 g
Mass of solution = 220 g
The solute in 220 g is 45.09 g
220 g = 2.22 × 45.09
In 100 g solution amount of solute:
45.09 g/2.22 = 20.3 g
Thus m/m% = 20.3 % NaCl
The noble gas that precedes a given partial electron configuration must <em>itself </em>have an electron configuration that is complete <em>up to </em>the partial electron configuration. The noble gas's electron configuration should, when fully written out right before the partial electron configuration, give us a valid electron configuration for some element.
For the first series, the highest principal energy level has the number 4, so our noble gas should <em>at least </em>be one that is in the third period (numerically, the energy level is the same as the period number). That noble gas would be argon. The partial electron configuration given is not that of a noble gas (note: all noble gases have an electron configuration that contains <em>N</em>p⁶, where <em>N </em>= the highest principal energy level). So, the noble gas that appropriately precedes our first partial electron configuration is [Ar].
Argon's electron configuration is 1s²2s²2p⁶3s²3p⁶. Using the Aufbau Principle, 4s² would correctly follow 3p⁶. [Ar]4s²3d¹⁰4p² is equivalent to writing out 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p²; either way, this would happen to be the electron configuration of germanium.
Now that we hopefully have our fundamentals down, we can apply them to figure out the noble gases that precede the remaining partial electron configurations.
[Kr]5s²4d¹⁰5p⁵: This is the electron configuration of iodine.
[He]2s²2p⁵: This is the electron configuration of fluorine.
[Xe]6s²4f¹⁴5d¹⁰6p²: This is the electron configuration of lead.
[Ne]3s²2: This is the electron configuration of magnesium.
