Carbonate is a polyatomic ion whose oxidation number is -2. How many carbonate ions would be required to bond with aluminum in a neutral ionic compound?
Carbonate is a polyatomic ion whose oxidation number is -2. How many carbonate ions would be required to bond with aluminum in a neutral ionic compound?
Oxidation number of each atom in sodium hydrogen carbonate ( NaHCO3) are
Na = +1
H = +1
C = +4
O = -2
Explanation:
Let's pick the first atom
NaHCO3
find oxidation number of Na
Na + 1 +4 + 3(-2) = 0( because there is no charge)
Na + 5 - 6 = 0
Na = 6 -5
Na = +1
Always put the sign
Find the oxidation number of H in NaHCO3
+1 + H + 4 + 3(-2) = 0.
H + 1 + 4 + 3(-2) = 0
H + 5 -6 = 0
H = 6 -5
H = +1
Find the oxidation number of C In NaHCO3
+1 +1 +C + 3(-2) = 0
C + 1+1-6 = 0
C +2 - 6= 0
C = 6 -2
C = +4
Find the oxidation number of O in NaHCO3
+1 + 1 + 4 + 3(O) = 0
6 + 3 (O) = 0
3(O) = -6
Divide through by 3 to get O
3(O) / 3 = -6 / 3
O = -6/3
O = -2
-2
Explanation:
carbonate oxifation number is -2
Part A: Hexacyanoferrate (III)
Part B: (II)
Part C: Dichlorobis(ethylenediamine) Chromate (II)
Part D: Triaquocarbonylnickel (II) Sulphate
Part E: Potassium (II)
Explanation:
For naming the complex ions there is a specific rule
Nomenclature of the complex ions are as follow
write a correct formulaeIndicate the oxidation number of metal in the complexThe oxidation number should write in the roman numeral in perenthasis after metal nameLigand named before the metal ionLigan can be named in following order
* 1st negative, 2nd neutral, 3rd positive
* If there are more than 2 same charged ligand the write in
alphabetical order.
Write prefix i.e di, tri, tetra for multiple monodentate ligandsAnions name end at ido the replace the final name.Neutral ligands named as their usual name, but there are some exceptions such as
NH3 named as ammine
H2O names aqua or aquo
CO named ascarbonyl
NO named as nitrosyl
If the complex is an anion, then name of the central atom will end in -ate, and its Latin name will be used except for mercuryThe name of full complex will end with cation or anion with separate word.
Keeping the rules in mind the complexes named as following.
Part A:
[Fe(CN)₆]³⁻
Name of the Complex : Hexacyanoferrate (III)
Part B:
[Cu(NH₃)₂(H₂O)₄]²⁺
Name of the Complex : (II)
Part C
CrCl₂(en)₂
Name of the Complex : Dichlorobis(ethylenediamine) Chromate (II)
Part C
[Ni(H₂O)₃(CO)]SO₄
Name of the Complex : Tetraaquocarbonylnickel (II) Sulphate
Part E
K₄[Pt(CO₃)₂F₂]
Name of the Complex : Potassium (II)
Three carbonate ions are required to bond with aluminum in a neutral ionic compound.
Explanation:
An ionic compound is defined as the compound that is formed by the complete transfer of electrons takes place from one atom (forming cation) to another atom (forming anion).
A neutral ionic compound does not carry any charge on it.
As we know, aluminum is a trivalent atom having valency 3 and forms [tex]Al^{3+}[/tex] ion and carbonate is a divalent polyatomic ion having formula [tex]CO_3^{2-}[/tex].
They both combine to form a neutral ionic compound named aluminum carbonate.
By criss cross method, the chemical formula of aluminum carbonate is [tex]Al_2(CO_3)_3[/tex]
Hence, three carbonate ions are required to bond with aluminum in a neutral ionic compound.
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2
3
4
5
Explanation:
2.)
a.) As we progress across the reaction scheme from methane to carbon dioxide, the carbon atom is being oxidized at every step of the way. In general terms, oxidation is the loss of electrons that leads to a higher oxidation state. In organic chemistry, the same principles apply, however, we typically mean forming more bonds to oxygen when referring to oxidation with these molecules. As we progress from methane to carbon dioxide, the central carbon atom is gaining a new bond to oxygen in each molecule. As carbon gains a bond to oxygen, its oxidation state increases by 2.
In CH₄, the oxidation state of carbon is -4. As we add a bond to oxygen to form CH₃OH, the oxidation state becomes -2. Adding another bond to oxygen to get formaldehyde, HCOH, gives carbon an oxidation state of 0. This trend continues as we form three bonds to carbon in formic acid, where the carbon has an oxidation state of +2, and finally the carbon has an oxidation state of +4 in carbon dioxide.
b.) Formaldehyde could be used as a molecule that can either be oxidized or reduced. We just demonstrated that the oxidation state of carbon can range from -4 to +4. The central carbon of formaldehyde has an oxidation state of 0, therefore, it could be readily oxidized or reduced as it falls in the middle of the possible oxidation states of carbon.
c.) Based purely on the oxidation states, and not on the real world reactivities of these molecules, the molecule that would be most likely to be reduced would be carbon dioxide. The carbon atom of CO₂ has an oxidation state of +4. Therefore, it cannot be oxidized any further and can only be reduced.
d.) Again, based purely on these oxidation states, methane is the most likely candidate to be oxidized. The carbon at of methane has an oxidation state of -4, making it the lowest oxidation state possible for carbon. This carbon atom can only be oxidized further.
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Artificial diamonds are made using thallium carbonate. If thallium has an oxidation number of 1+ number 2 A chemical bond is a lasting attraction between atoms, ions or molecules that enables the formation of chemical compounds. The bond may result from the electrostatic force of attraction between oppositely charged ions as in ionic bonds or through the sharing of electrons as in covalent bonds. number 3 giant metallic, giant ionic, simple molecular, and macromolecular ... it has positive ions surrounded by a sea of delocalised electrons ... m/z value than Cl⁻. this means that F⁻ is more attracted to the Ca²⁺ ion more strongly ... What bond angle does beryllium chloride, BeCl₂ have? ... Give two examples of linear molecules.
1. D (24.0 moles CO2)
2. A (.239 moles H2)
Explanation:
1. First Balance the equation
1 C3H8 + 5 O2 ---> 3 CO2 + 4 H2O
Then set up a stoiciometric equation so that the moles of O2 cancel out
40mol O2 x [tex]\frac{3 mole CO2}{5 mole O2}[/tex] = 24.0 moles CO2
2. Set up a stoichiometric equation
10 grams Fe x [tex]\frac{1 mole Fe}{55.85 grams Fe}[/tex] x [tex]\frac{4 mole H2}{3 mole Fe}[/tex] = 0.239 moles H2