1. Magnesium atoms also have a slightly smaller radius than sodium atoms, and so the delocalised electrons are closer to the nuclei.
2. Sodium has higher melting point than potassium because of stronger metallic bonding .
3. Potassium are very soft metal can be very easily cut with a knife
4. Increase of resistance in metals. Therefore the mobility of electrons decreases and causes decrease in conductivity.
5.To increase strength, increase corrosion resistance, or reduce costs.
6. All metals have low ionization energies and are relatively electropositive, and so they lose electrons fairly easily.
7. All the group 1 metals are reactive, but they get more reactive as you go down the group, so potassium is more reactive than sodium.
The best answer among the following choices would be A) since the other options are NOT nonrenewable energy sources.
Are you talking about the starch idione test? Because you didnt ask what the actual question was?
Answer:
<em>Rate constants are temperature dependent.</em>
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Explanation:
Reaction rate is used to quantify the rate of chemical reaction. There is a relationship between the reaction rate and the half-life of the reaction and the Gibbs free energy of activation, and the reaction rate is temperature dependent according to the equation.
For a reaction shown below
a A + b B ⇒ c C
The rate of reaction of the reaction is given by
where k(T) is the reaction constant, which is seen to be dependent on the temperature of the reaction.
Also, k(T) is numerically equal to
where
r = reaction rate
A = pre exponential factor
= Activation energy
R = gas constant
T = temperature
and m and n are experimentally determined partial orders in [A] and [B]
Explanation:
In balancing chemical equations, the law of conservation of matter must be strictly obeyed.
By the virtue of this, the following steps are usually taken:
- First identify the atoms on each side of the expression. This to know the number of species to balance.
- Then count the atoms on each side.
- Then using appropriate number as the coefficients, increase the atom on each side until there are equal numbers on both sides.
- Finally, check to make sure we have the same number of each type of atom on each side.