<span>Cleavage because the thin sheets will break apart easily in one direction but not the other.</span>
Atomic mass of boron = 10.81
<h3>What are Isotopes?</h3>
Isotopes are variants of a particular element in which they have the same number of protons but differ in the number of neutrons in the atom.
So, here as we said we have isotopes which weigh 10.01 and 11.01.
Given,
relative abundance of B-10 = 10.1 amu
relative abundance of B- 11 = 11.01 amu
percentage of B-10 = 20%
percentage of B-11 = 80%
Then the relative atomic mass depends upon the relative abundance of various isotopes of that particular element. Suppose an element consists of two isotopes and average atomic mass is equal to
(Relativeabundance(1)×Atomicmass(1)+Relativeabundance(2)×Atomicmass(2)) / (Relativeabundance(1)+Relativeabundance(2))
Atomic mass of boron = (20 × 10.01 + 80 × 11.01) / (80 + 20 )
= 1081/100
= 10.81
To learn more about atomic mass from the given link
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Answer:
1
Explanation:
The empirical formula describes the simplest whole number ratio of each type of atom in a compound. To find this formula, you need to (1) convert grams of each element to moles (via their atomic masses) and then (2) find the ratio of each element (by dividing each molar value by the smallest mole value).
(Step 1)
Atomic Mass (Zn): 65.380 g/mol
Atomic Mass (C): 12.011 g/mol
Atomic Mass (O): 15.998 g/mol
10.40 grams Zn 1 mole
------------------------ x ------------------------ = 0.159 moles Zn
65.380 grams
1.92 grams C 1 mole
--------------------- x ----------------------- = 0.160 moles C
12.011 grams
7.68 grams O 1 mole
---------------------- x ------------------------ = 0.480 moles O
15.998 grams
(Step 2)
0.159 moles Zn / 0.159 = 1 atom Zn
0.160 moles C / 0.159 = 1 atom C
0.480 moles O / 0.159 = 3 atom O
The empirical formula is Zn₁C₁O₃. Therefore, the value that should be in the space is 1.
Answer:
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Explanation:
2 Atom of Hydrogen are present in 2 (NaHCO3)
