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Chemcial Equation: C3H8 + O2 ( CO2 + H2O
If 50.0 grams of Cl2 gas is reacted with enough sodium hydroxide (NaOH), calculate the following:
Mass in grams of sodium hypochlorite (NaOCL) produced
Moles of sodium chloride (NaCl) produced
Chemical Equation: NaOH + Cl2 ( NaOCl + NaCl + H2O
Calculte the number of moles in200g of O gas
I am trying to understand electron configuration backfilling because I see that there is 2,8,16,2 for NI then it skips to 2,8,18,1 for CU
some say CU is 2, 8, 18, 1 and others say CU is 2, 8, 17, 2
Then I heard the atoms holds 8 electrons and fills 17 (What is the difference between hold and fill)
also don't see how the 3rd row when move it up to the 3rd row, how the numbers fit in sequence?
- From 1 part of the question, which is the hold and fill. I think it means that to fill would be referring to bonding with other atoms
- but then again according to this definition I still don't understand: A stable arrangement is attended when the atom is surrounded by eight electrons. This octet can be made up by own electrons and some electrons which are shared. Thus, an atom continues to form bonds until an octet of electrons is made. This is known as octet rule by Lewis.
If I have electron configuration, I have to fill 4s first then 3d. Does that mean 4s energy is lower than 3d? Also, does that mean that in the 4th shell electron orbit the atom will receive 2 electrons first (due to fulfill the 4s subshell) and then fill 10 electrons into the 3rd atomic shell (due to fulfill the 3d subshell)? Thank you.
A 0.415 g sample of KHP will be titrated with a NaOH solution with an assumed concentration of 0.100 M.
Calculate the volume of NaOH that should neutralize the KHP sample.
Complete this table to show the pH and pOH of each solution.
(H+ is short for H3O+)
[H+] [OH−] pH pOH
Solution A 1.0×10−5 5
Solution B 1.0×10−10 10
Solution C 1.0×10−12
Solution D 10
Solution A [OH−]=
M
Solution A pOH=
Solution B [H+]=
M
Solution B pH=
Solution C [OH−]=
M
Solution C pH=
Solution C pOH=
Solution D [H+]=
M
Solution D [OH−]=
M
Solution D pOH=
Calculate the [OH−] and the pH of a solution with an [H+]=4.0×10−13 M at 25 °C .
[OH−]=
pH=
Calculate the [H+] and the pH of a solution with an [OH−]=9.8×10−13 M at 25 °C .
[H+]=
pH=
Calculate the [H+] and the [OH−] of a solution with a pH=3.52 at 25 °C .
[H+]=
[OH−]=
Explain why electron affinity decreases down the group
25.7 ml of 0.487 M HCl and 15.4 ml of 0.765 ml NaOH are mixed.
Determine the mmol of HCl and NaOH in the two solutions that are being mixed.
mmol HCl
mmol NaOH
Which reactant is present in excess?
Is the solution acidic, basic or neutral?
25.7 ml of 0.487 M HCl and 15.4 ml of 0.765 ml NaOH are mixed.
Determine the mmol of HCl and NaOH in the two solutions that are being mixed.
Which reactant is present in excess?
Is the solution acidic, basic or neutral?
