Answer:
Lithium is more reactive as it has only one electron in its valance shell. Beryllium has 2 valance electrons. Lithium is more reactive as it is easier to lose oneelectron than losing two electrons.
Answer:
it would take longer to boil on top of a mountain because the water is not as hat
1. Compared to oxygen, nitrogen's __________ makes it more difficult for water molecules to the surround nitrogen molecules.
<span>2. The high solubility of sulfur dioxide can be explained by its ____________. </span>
<span>3. Nitric oxide is more soluble than nitrogen and oxygen because of its _______________. </span>
<span>4. Compared to nitrogen, the ___________ of ethylene makes it more soluble in water. </span>
<span>CHOICES are: </span>
<span>a. shorter bond length </span>
<span>b. ability to react with water </span>
<span>c. larger molecular size </span>
<span>d. polarity
answers: </span><span>a, b, d, c.</span><span>
</span>
Answer:
2H2O2(aq)→ 2H2O(l) O2(g) : The oxidation number of oxygen for each compound is -1, -2, 0
Explanation:
In peroxides the oxidation state of oxygen is -1, since one oxygen bonds to the other oxygen and a hydrogen and the bound oxygen captures the electron of the remaining hydrogen. Through a scheme would be
H --- O --- O --- H
We remember that oxygen needs two electrons to get to have the configuration of the nearest noble gas (Lewis octet rule). In Peroxides, the oxygen is linked by covalent bonds. If we take it strictly, peroxide is a grouping of two oxygen, having the whole valence -2. which is why it is usually said that it is when oxygen has a valence -1
As we said the oxidation state is -2, the one that appears in the water molecule, since Hydrogen acts with valence +1 and it is 2 atoms that give up electrons to compensate for oxygen.
In the O2 it acts with valence 0 since we talk about gas in its elementary state. All diatomic molecules in their elemental state, generally gases or metals in solid state, act with a valence of 0.
As you go across a period, radius shrinks because you are adding protons. The added positive charge increases pull on the electron shells.
As you go down a group, radius gets larger because you are increasing shells of electrons. This increases shielding of the nucleus' positive charge, so the electrons are not pulled in as much.
