Answer:
3.14
Explanation:
A student was comparing two samples with an equal number of carbon atoms. One sample contained only Carbon-12 atoms. One sample contained only Carbon-14 atoms, which contain two more neutrons than Carbon-12 atoms. The student measured the mass of each sample and testing the reactivity of each sample.
Required:
What would best describe the results of the investigation?
Answer: Option (b) is the correct answer.
Explanation:
In a chemical reaction, the bonds between the reactant molecules tend to break leading to the formation of new bonds to produce products.
So, in order to break the bonds between the reactant molecules, energy is required to overcome the attraction between the atoms.
To form new bonds, energy gets released when two atoms come closer to each other. Hence, formation of bond releases energy.
As in the given reaction it is shown that 
< 0, that is, enthalpy change is negative. Hence, energy is released as it is an exothermic process.
Thus, we can conclude that the statement energy released as the bonds in the reactants is broken is greater than the energy absorbed as the bonds in the products are formed, is true about the bond energies in this reaction.
Answer:
1,2,1,2
Explanation:
You would need only one of the CH4 but 2 of the O2 then 1 CO2 and 2 H2O on each side of the equation you now have 1 carbon, 4 hydrogen, and 4 oxygen.
Answer:
The orbital notations shows the sequence of filling electrons into the orbitals of sublevels. This filling is based on some certain principles. For an atom with 16 electrons, the orbital diagram is shown below: 1s²2s²2p⁶3s²3p⁴ The maximum number of electrons in each sublevel of the orbitals are: 2 electrons for s-sublevel with one orbital
6 electrons for p-sublevel with three orbital
10 electrons for d-sublevel with five orbital
14 electrons for f-sublevel with seven orbital
According to the Aufbau's principle, sublevels with lower energy are filled before those with higher energy.
1s 2s 2p 3s 3p 4s 3d etc
Pauli's exclusion principle shows that no two electrons can have the same set of values for the four quantum numbers. Simply, no two electrons can spin in the same direction. Hund's rule states that electrons go into degenerate orbitals of sub-levles(s,p,d and f) singly before pairing commence. This rule shows that in each energy level, as the electron goes into the degenerate orbitals, they fill it one by one before they begin to pair up. As we know, each degenerate orbital can only accomodate 2 electrons. From the orbital diagram 1s²2s²2p⁶3s²3p⁴, the 3p sublevel has 3 orbitals. In each of the orbitals, two electrons would occupy them to give a maximum capacity of 6. But the sublevel has just 4 electrons. Based on Hund's rule, an electron will go into each of the 3 orbitals first. The remaining electron will now pair with the first degenerate orbital. This makes a total of 4 electrons.
Explanation:
