Answer: As a result, each excited electron in an atom emits a photon of a specific wavelength. To put it another way, each excited noble gas emits a distinct hue of light. This is a reddish-orange neon light.
Answer:
Approximately
under standard conditions.
Explanation:
Equation for the overall reaction:
.
Write down the ionic equation for this reaction:
.
The net ionic equation for this reaction would be:
.
In this reaction:
- Zinc loses electrons and was oxidized (at the anode):
. - Copper gains electrons and was reduced (at the cathode):
.
Look up the standard potentials for each half-reaction on a table of standard reduction potentials.
Notice that
is oxidation and is likely not on the table of standard reduction potentials. However, the reverse reaction,
, is reduction and is likely on the table.
The reduction potential of
would be
, the opposite of the reverse reaction
.
The standard potential of the overall reaction would be the sum of the standard potentials of the two half-reactions:
.
It can change in C. compounds to change when elements combine that will form
Answer:
(A) a compound that donates protons
.
Explanation:
According to Bronsted-Lowry Model
:
- Bases are proton acceptors.
(A) a compound that donates protons
.