Answer:
1.59mol/L
Explanation:
Data obtained from the question include:
Mass of MgCl2 = 151g
Volume of water(solvent) = 1L
Now, let us calculate the number of mole of MgCl2. This is illustrated below:
Molarity Mass of MgCl2 = 24 + (2x35.5) = 24 + 71 = 95g/mol
Mass of MgCl2 = 151g
Number of mole of MgCl2 =?
Number of mole = Mass /Molar Mass
Number of mole of MgCl2 = 151/95
Number of mole of MgCl2 = 1.59mole
Now we can calculate the molarity of MgCl2 as follow:
Mole = 1.59mole
Volume = 1L
Molarity =?
Molarity = mole /Volume
Molarity = 1.59/1
Molarity = 1.59mol/L
Answer is: <span>unbalanced electronegativity of the hydrogens and oxygens as they share electrons.
Oxygen has greater electronegativity than hydrogen, because of that oxygen is partially negative and hydrogen is partially positive.
</span>Electronegativity<span> is a </span>chemical property<span> that describes the tendency of an </span>atom<span> to attract a shared pair of </span>electrons<span> towards itself.</span>
I think you means the KO2 reacts with H2O. The equation of this reaction is 4KO2+2H2O->4KOH +3O2. The ratio of mole number of O2 and KO2 is 3:4. So the mole number of O2 produced is 0.500/4*3=0.375 mol.
Answer:
The atomic mass of phosphorus is 29.864 amu.
Explanation:
Given data:
Atomic mass of phosphorus = ?
Percent abundance of P-29 = 35.5%
percent abundance of P-30 = 42.6%
Percent abundance of P-31 = 21.9%
Solution:
Average atomic mass = (abundance of 1st isotope × its atomic mass) +(abundance of 2nd isotope × its atomic mass) + (abundance of 3rd isotope × its atomic mass / 100
Average atomic mass = (29×35.5)+(30×42.6) + (31×21.9) /100
Average atomic mass = 1029.5 + 1278 + 678.9/ 100
Average atomic mass = 2986.4 / 100
Average atomic mass = 29.864 amu.
The atomic mass of phosphorus is 29.864 amu.
Answer: 
Explanation:
Principle Quantum Numbers : It describes the size of the orbital and the energy level. It is represented by n. Where, n = 1,2,3,4....
Halogen with n=3 is chlorine.
Alkaline earth metal with n = 4 is calcium.
An ionic bond is formed when an element completely transfers its valence electron to another element.
Electronic configuration of calcium
![[Ca]=1s^22s^22p^63s^23p^64s^2](https://tex.z-dn.net/?f=%5BCa%5D%3D1s%5E22s%5E22p%5E63s%5E23p%5E64s%5E2)
calcium atom will loose one electron to gain noble gas configuration and form calcium cation with +2 charge.
![[Ca^{2+}]=1s^22s^22p^63s^23p^6](https://tex.z-dn.net/?f=%5BCa%5E%7B2%2B%7D%5D%3D1s%5E22s%5E22p%5E63s%5E23p%5E6)
Electronic configuration of chlorine:
![[Cl]=1s^22s^22p^63s^23p^5](https://tex.z-dn.net/?f=%5BCl%5D%3D1s%5E22s%5E22p%5E63s%5E23p%5E5)
Chlorine atom will gain one electron to gain noble gas configuration and form chloride ion with -1 charge.
![[Cl^-]=1s^22s^22p^63s^23p^6](https://tex.z-dn.net/?f=%5BCl%5E-%5D%3D1s%5E22s%5E22p%5E63s%5E23p%5E6)
Here 
cation and chloride 
anion combine and their oxidation states are exchanged and written in simplest whole number ratios to give neutral .
