Answer:
1G
Explanation:
U ever get an answer
The city council of a small town wanted to add fluoride to their water so that all the residents would have healthier teeth. The mayor had read that ionic compounds must be used to get the fluoride into water. He looked up fluorine-containing compounds and came up with the following list.
NaF NF3 SiF4 CaF2 NH4F
Using academic vocabulary in paragraph form, discuss the following:
Explain which compound(s) could produce fluoride ions in the water. In your response, be sure to include:
° which of the listed compounds are ionic and which are covalent.
° how ionic and covalent compounds are different.
° why only ionic compounds would produce fluoride in water.
Answer:NaF is ionic. NF3 is covalent. SiF4 is ionic. CaF2 is Ionic and NH4F is also ionic. Ionic compounds transfer electrons whereas covalent compounds share electrons hence the word "co". Also, ionic compounds are formed with metal and nonmetal. Where a covalent is with 2 nonmetals. Only ionic compounds would produce fluoride in water because ionic compounds can dissolve in water and covalent compounds cant.
The compounds that can be used for the release of fluorine in water are NaF, [tex]\rm SiF_4[/tex], [tex]\rm CaF_2[/tex], and [tex]\rm NH_4F[/tex].
The ionic compounds are formed by the transfer of electrons between the atoms of the compounds. The ionic bonds are weaker and are easy to dissociate in the aqueous solution.
The covalent compounds are formed by the sharing of electrons between the atoms. Since there is sharing, there has been a strong bond, that has been hard to dissociate.
The Mayor has to release Fluoride in the water, thus ionic compounds are preferred that have the easy release of fluorine.
From the given compounds:
NaF = Ionic compound[tex]\rm NF_3[/tex] = Covalent compound[tex]\rm SiF_4[/tex] = Ionic compound[tex]\rm CaF_2[/tex] = Ionic compound[tex]\rm NH_4F[/tex] = Ionic compoundThus the compounds that can be used for the release of fluorine in water are NaF, [tex]\rm SiF_4[/tex], [tex]\rm CaF_2[/tex], and [tex]\rm NH_4F[/tex].
For more information about ionic and covalent compounds, refer to the link:
https://brainly.com/question/10748806
how do you separate the following mixture? Name only the process involved .
1.Sand and salt
Answer:
Just dissolve in water , you can separate
Explanation:
because salt dissolves in water but sand doesn't
Explanation:
sedinentation and decantation
Your private gas collection consists of the four following gases, with each gas in a separate container, and exactly 1.0 g of each gas: CO2(g). Ne (g), Cl2
(g), and H2S (g). Which of your prized gases occupies the smallest volume at standard temperature and pressure (STP)?
H2S (g)
CO2 (g)
Cl2 (g)
Ne (g)
Answer:Cl2
Explanation:each gas is 1 gm and has the same P andT. The gas with the highest molar mass will have the lowest volume with least moles. Cl2 wins the prize
Using the bond energies provided, calculate the enthalpy of the reaction (∆Hrxn, in kJ) for the hydrogenation of propene to propane, shown below?
CH₂CHCH₃(g) + H₂(g) → CH₃CH₂CH₃(g)
The enthalpy of reaction for the hydrogenation of propene to propane is -926 kJ/mol.
The bond energy of a molecule is obtained as the sum of the bond energies of all the bonds between atoms in the molecule. The heat of reaction can be obtained using the relation;
∆Hrxn = ∑Bonds being broken - ∑Bonds being formed
Hence, we have;
Where all the energies are quoted in KJ/mol
C=C = 598
C - C = 346
H - H = 436
C - H = 416
For the reaction;
CH₂CHCH₃(g) + H₂(g) → CH₃CH₂CH₃(g)
∆Hrxn = ∑[6(C - H) + 1(C=C) + 1(C - C)] - ∑[3(C - C) + 8(C - H)
∆Hrxn = [6(416) + 1(598) + 1(346)] - [3(346) + 8(416)]
∆Hrxn =3440 - 4366 = -926 kJ/mol
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