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vazorg [7]
2 years ago
7

Arrange the following bonds in order of increasing ionic character. assign number 1 as the highest and 6 as the lowest. a. carbo

n-hydrogen
b. fluorine-hydrogen
c. bromine-hydrogen
d. sodium-chlorine
e. potassium-fluorine
f. lithium-chlorine
Chemistry
1 answer:
SIZIF [17.4K]2 years ago
5 0
Answer: Potassium to fluorine, fluorine to nitrogen, bromine to hydrogen, carbon to hydrogen, lithium to chlorine, sodium to chlorine.
Explanation:
Ionic bond is greater when the electronegativity difference existing between the two atoms are large causing the bonding to be more polar.
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a helium balloon has a volume of 2.95 liters at 25 c. the volume of the ballon decreased to 2.25 l after it is placed outside on
OleMash [197]

Answer:

The outside temperature is -45.8°C

Explanation:

When a gas keeps on constant its moles and its pressure, we can assume that volume will be increased or decreased as the T° (absolute T° in K).

V1 / T1 = V2 / T2

2.95L/298K = 2.25L / T2

(2.95L/298K ) . T2 = 2.25L

T2 = 2.25L . 298K / 2.95L

T2 = 227.2K

T°K - 273 = T°C

227.2K - 273 = -45.8°C

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3 years ago
A gecko used its sticky feet to crawl from the bottom of a window to the top of
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8 0
3 years ago
When carbon is burned in air, it reacts with oxygen to form carbon dioxide. When 14.4 g of carbon were burned in the presence of
Natasha2012 [34]

When carbon reacts with oxygen it forms CO2. This can depicted by the below equation.

C + O2→ CO2

It has been mentioned that when 14.4 g of C reacts with 53.9 g of O2, then 15.5 g of O2 remains unreacted. <u>This indicates that Carbon is the limiting reagent and hence the amount of CO2 produced is based on the amount of Carbon burnt.</u>

C + O2→ CO2

In the above equation , 1 mole of carbon reacts with 1 mole of O2 to produce 1 mole of CO2.

In this case 14.4 g of Carbon reacts with 53.9 of O2 to produce "x"g of CO2.

<u>No of moles = mass of the substance÷molar mass of the substance</u>

No of moles of carbon = 14.4 /12= 1.2 moles

No of moles of O2 = Mass of reacted O2/Molar mass of O2.

No of moles of O2 = (Total mass of O2 burned - Mass of unreacted O2)/32

No of moles of O2 = (53.9-15.5) ÷ 32 = 1.2 moles.

Hence as already discussed 1 mole of Carbon reacts with 1 mole of O2 to produce 1 mole of CO2. In this case 1.2 moles of carbon reacts with 1.2 moles of O2 to produce 1.2 moles of CO2.

Moles of carbon dioxide = Mass of CO2 produced /Molar mass of CO2

Mass of CO2 produced(x) = Moles of CO2 ×Molar mass of CO2

Mass of CO2 produced(x) = 1.2 x 44 = 52.8 g

<u>Thus 52.8 g of CO2 is produced.</u>

5 0
3 years ago
Why is molybdenum a good conductor of electricity
SCORPION-xisa [38]

Answer: Because it is has a strong connection

Explanation:

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Consider the diagram below
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Energy of the reactants would be correct
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