Ionic bonds are made up of a metal and a nonmetal elements while covalent bonds are are made up of two metal. So, you can just look at the periodic table and identify which compounds have two metals and which have one metal and one nonmetal. Also, those compounds with high electronegativity difference are very likely to be ionic while the opposite is covalent. HOWEVER, some compounds can be both covalent and ionic. For instance, if HCI gas is at higher temperatures, then it is ionic while it would be covalent at room temp.
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Answer:
A
Explanation:
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Answer:
D. 9.0x10²³ atoms
Explanation:
First we use <em>Avogadro's number</em> to <u>calculate how many molecules of Si₂H₆ are there in 0.75 mol</u>:
- 0.75 mol * 6.023x10²³ molecules/mol = 4.52x10²³ molecules
There are 2 Si atoms in one Si₂H₆ molecule, that means that in 4.52x10²³ Si₂H₆ molecules there will be:
- 2 * 4.52x10²³ = 9.03x10²³ Si atoms
Thus the answer is option D.
Answer:
A. volume
Explanation:
Generally the equation for the ideal gas is mathematically given as
PV=nRT
Where
P=pressure
V=volume
R=gas constant
n=Number of Moles
T=Temperature
Therefore
V=nRT/P
Option A
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Answer:
The Ka is 9.11 *10^-8
Explanation:
<u>Step 1: </u>Data given
Moles of HX = 0.365
Volume of the solution = 835.0 mL = 0.835 L
pH of the solution = 3.70
<u>Step 2:</u> Calculate molarity of HX
Molarity HX = moles HX / volume solution
Molarity HX = 0.365 mol / 0.835 L
Molarity HX = 0.437 M
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<u>Step 3:</u> ICE-chart
[H+] = [H3O+] = 10^-3.70 = 1.995 *10^-4
Initial concentration of HX = 0.437 M
Initial concentration of X- and H3O+ = 0M
Since the mole ratio is 1:1; there will react x M
The concentration at the equilibrium is:
[HX] = (0.437 - x)M
[X-] = x M
[H3O+] = 1.995*10^-4 M
Since 0+x = 1.995*10^-4 ⇒ x=1.995*10^-4
[HX] = 0.437 - 1.995*10^-4 ≈ 0.437 M
[X-] = x = 1.995*10^-4 M
<u>Step 4: </u>Calculate Ka
Ka = [X-]*[H3O+] / [HX]
Ka = ((1.995*10^-4)²)/ 0.437
Ka = 9.11 *10^-8
The Ka is 9.11 *10^-8