Which of the following is considered a strong acid HF, HClO4, H3PO4, or HC2H3O2

Predict the geometry around the central atom in SO2- A) trigonal pyramidal B) tetrahedral C) octahedral D) trigonal planar E) tr

liubo4ka [24]

Answer: The correct answer is Option D.

Explanation:

To calculate the hybridization of $SO_2$ , we use the equation:

$\text{Number of electron pair}=\frac{1}{2}[V+N-C+A]$

where,

V = number of valence electrons present in central atom (S) = 6

N = number of monovalent atoms bonded to central atom = 0

C = charge of cation = 0

A = charge of anion = 0

Putting values in above equation, we get:

$\text{Number of electron pair}=\frac{1}{2}[6]=3$

The number of electron pair around the central metal atom are 3. This means that the hybridization will be $sp^2$ and the electronic geometry of the molecule will be trigonal planar.

Hence, the correct answer is Option D.

3 0

3 years ago

Equation balancing

meriva

Answer:

For a: The balanced equation is $2S(s)+3O_2(g)\rightarrow 2SO_3(g)$

For c: The balanced equation is $2NaOH(s)+H_2SO_4(aq)\rightarrow Na_2SO_4(aq)+2H_2O(l)$

Explanation:

A balanced chemical equation is one where all the individual atoms are equal on both sides of the reaction. It follows the law of conservation of mass.

For (a):

The given unbalanced equation follows:

$S(s)+O_2(g)\rightarrow SO_3(g)$

To balance the equation, we must balance the atoms by adding 2 infront of both $S(s)$ and $SO_3$ and 3 in front of $O_2$

For the balanced chemical equation:

$2S(s)+3O_2(g)\rightarrow 2SO_3(g)$

For (b):

The given balanced equation follows:

$2Al(s)+3Cl_2(g)\rightarrow 2AlCl_3(s)$

The given equation is already balanced.

For (c):

The given unbalanced equation follows:

$2NaOH(s)+H_2SO_4(aq)\rightarrow Na_2SO_4(aq)+H_2O(l)$

To balance the equation, we must balance the atoms by adding 2 infront of $H_2O(l)$

For the balanced chemical equation:

$2NaOH(s)+H_2SO_4(aq)\rightarrow Na_2SO_4(aq)+2H_2O(l)$

For (d):

The given balanced equation follows:

$C_3H_8(g)+5O_2(g)\rightarrow 3CO_2(g)+4H_2O(g)$

The given equation is already balanced.

4 0

3 years ago

I need Helpppp with my chemistry while we are out of school. I don't have a good teacher and he's not helping since it's his las

9966 [12]

Answer:

im not sure but I hope this helps

Explanation:

I believe the equivalents is just the moles reactant/moles limiting reactant

water has a denisty of 1 g/mL. 1 L is 1000 ml so there are 1000g/L.

the molar mass of water is 18g/mol if you use the Liters in the equation above you can find the number of grams present. divide this number you found by 18 to find the moles.

now take the amount of the other reactant given and divide it by its own molar mass. this will give you the number of moles of that reactant.

divide the moles of water by the moles of the reactant and that is the equivalent.

to find the normality you take this number and divide it by the number of liters.

5 0

3 years ago

PLEASE ANSWER IM ON A TIME LIMIT PLEASEEEE: Comparative investigations: collecting data for blank

jarptica [38.1K]

Observation, I think

6 0

3 years ago

Choose the molecule or compound that exhibits dipole-dipole forces as its strongest intermolecular force.

LuckyWell [14K]

Answer:

SO2

Explanation:

Dipole-Dipole exist between parmanent dipoles in a molecule. THis means that molecule must have a parmanent dipole moment in it.

Example - HCl

Hydrogen bonding is an attraction between lone pair of an electronegative element and H atom of same or different molecule. H must be covalantly attached to either F, N or O.

Example - H2O

Among the molecules given in the list only SO2 and H2O exihibits parmanent moment. As BCl3 , CBr4 and H2 are symmetric compounds.

Since, SO2 cannot exihibit H- bonding only dipole-dipole forces as its strongest intermolecular force.

5 0

3 years ago