Answer:
Elements only contain one type of atoms while compounds contain two or more types of atoms.
Explanation:
An example of an element is sodium --> Na (only Na atoms)
An example of a compound can be water --> H2O (contain H and O atoms)
*But the particles within a compound are all the same.
Answer:
1.66 × 10⁻¹⁸ Moles
Explanation:
As we know one mole of any substance contains 6.022 × 10²³ particles (atoms, ions, molecules or formula units). This number is also called as Avogadro's Number.
The relation between Moles, Number of Atoms and Avogadro's Number is given as,
Number of Moles = Number of Atoms ÷ 6.022 × 10²³ Atoms/mol
Putting values,
Number of Moles = 1.0 × 10⁶ Atoms ÷ 6.022 × 10²³ Atoms/mol
Number of Moles = 1.66 × 10⁻¹⁸ Moles
Answer:
1) 262 grams
Explanation:
Mg = 24.305g
O = 16g
H = 1
24.305 +2(16)+2(1) = 58.305 g
×
Answer:
This is a ratio of two small integers, 1.500 = 3:2. Let's assume that in the molecule of ferrous oxide there is one oxygen atom and one iron atom, and the ratio of the mass of the oxygen atom to the mass of the iron atom is 0.2865.
Explanation:
Molecular weight of Iron (II) oxide= FeO Molecular weight of Iron (III) oxide= Fe2O3
In FeO , every one iron atom contains one oxygen atom.
In Fe2O3, every one iron atom contains 1.5 oxygen atoms.
So FeO(II) will contain more Iron than FeO(III).
Calculation of percentage of iron is not necessary. I think this argument
alone is enough to prove this.
However on calculating the % of Fe, in FeO and Fe2O3 we get,
% of Iron in FeO= 55.85/(55.85+16) =55.85/71.85= 77.73%
% of Iron in Fe2O3= (2 x55.85)/(111.7+48)
=111.7/159.48 = 69.94%
The polarity of a water molecule
comes from the uneven distribution of electron density of hydrogen and oxygen
atom. The oxygen in the water molecule is more electronegative than the
hydrogen. Water has a partial positive charge near the hydrogen atom and a
partial negative charge near the oxygen atom. The result of this
electrostatic attraction results in the bond called hydrogen bond. Also,
because of this bond, it has the ability to dissolve most of the solutes due to
its polarity and bonding.
