Answer:
- <u><em>Ratio of the mass carbon that combines with 1.00 g of oxygen in compound 2 to the mass of carbon that combines with 1.00 g of oxygen in compound 1 = 2</em></u>
Explanation:
First, detemine the mass of oxygen in the two samples by difference:
- mass of oxygen = mass of sample - mass of carbon
Item Compound 1 Compound 2
Sample 80.0 g 80.0 g
Carbon 21.8 g 34.3 g
Oxygen: 80.0 g - 21.8g = 58.2 g 80.0 g - 34.3 g = 45.7 g
Second, determine the ratios of the masses of carbon that combine with 1.00 g of oxygen:
- For each sample, divide the mass of carbon by the mass of oxygen determined above:
Sample Mass of carbon that combines with 1.00 g of oxygen
Compound 1 21.8 g / 58.2 g = 0.375
Compound 2 34.3 g / 45.7 g = 0.751
Third, determine the ratio of the masses of carbon between the two compounds.
- Divide the greater number by the smaller number:
- Ratio = 0.751 / 0.375 = 2.00 which in whole numbers is 2
The reason why it is not considered this is because the material was made in a lab, not through nature, which is what is required to be considered as a true mineral.
A covalent bond describes two atoms (most likely nonmetals) that share their valence electrons to satisfy the octet rule. Carbon and oxygen are both nonmetals, and they would share electrons with each other through a bond that is not polar enough to be considered ionic. The answer should be B
Noble Gas. Metals have 1 or 2 Valence Electrons. Halogens have 7 Valence Electrons. Semi-Metals can have different amounts.
Answer:
520ML and apparently I need to put more in this answer
Explanation:
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