Answer: The density of the unknown metal is 7.86 g/ml.
Explanation:
Density is defined as the mass contained per unit volume.
Given : Mass of metal = 25.32 g
Volume of metal = volume of water displaced = (28.22 - 25.00) ml = 3.22 ml
Putting in the values we get:
Thus the density of the unknown metal is 7.86 g/ml
- If the abundance of the first isotope is 68.037%, then the abundance of the second isotope is 100%-68.037%.
Substituting into the atomic mass formula,

<u>Ionic Bond</u> is formed when the electronegativity difference is 0.4 > 2.0. Electronegativity is a term that can be defined as a tendency of an atom to attract electron towards its own self.
Explanation:
Electronegativity is a term that can be defined as a tendency of an atom to attract electron towards its own self.
An electronegativity of an atom is affected by
- The atomic number of the atom
- Secondly by the distance at which the valence electron are residing from the nucleus
1. In case the electronegativity difference (which is denoted by ΔEN) is less than 0.5 then the bond formed is known as N<u>onpolar covalent.
</u>
2. In case the ΔEN is in between 0.5 and 1.6, the bond formed is referred to as the<u> Polar covalent
</u>
3. In case the ΔEN is more /greater than 2.0, then the bond formed is referred to as<u> Ionic Bond</u>
<u>2 Examples of Ionic bonds</u>
- The formation of sodium fluoride, NaF, from a sodium atom and a fluorine atom is an example of Ionic bond formation.
- Another example is the formation of NaCl from sodium (Na),which is a metal, and chloride (Cl), which is a nonmetal
6000 I pretty sure tell me if it's right
Data: molar mass 470 g/mol
Percent composition:
Hg = 85.0%
Cl = 15.0%
Solution:
1) Convert % to molar ratios
A. Base: 100 g
=> Hg = 85.0 g / 200.59 g/mol = 0.4235 mol
Cl = 15.0 g / 35.45 g/mol = 0.4231 mol
B. divide by the higher number and round to whole number
Hg = 0.4325 / 0.4231 = 1.00
Cl = 0.4231 / 0.4231 = 1.00
=> Empirical formula = Hg Cl
2) Find the mass of the empirical formula:
HgCl: 200.59 g/mol + 35.45 g/mol = 236.04
3) Determine how many times is the empirical mass contained in the molecular mass:
470 g/mol / 236.04 = 1.99 ≈ 2
=> Molecular formula = Hg2 Cl2.
Answers:
Empirical formula HgCl
Molecular Formula Hg2Cl2