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3 years ago

Reply ASAP: Why do electrons affect the structure of a molecule?

Chemistry

1 answer:

antoniya [11.8K]3 years ago

7 0

Answer:

C. The electron clouds are negatively charged and repel each other as far apart as possible

Explanation:

This is the basis of VSEPR theory.

The angles between the electron clouds determine the shapes of the molecules.

B. and D. are wrong. All electron pairs are negatively charged.

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Which of the following statements is BEST describes an abusive relationship? A. An abusive partner will admit to the problem and

Ray Of Light [21]

The answer would be:

C. The abuse will happen again regardless of how sorry the abuser seems to feel.

Hope this helps! :)

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3 years ago

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A trial of this decomposition experiment, using different quantities of reactants than those listed in the question above produc

Paul [167]

Answer : The volume of $O_2(g)$ produced at standard conditions of temperature and pressure is 0.2422 L

Explanation :

Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law.

The combined gas equation is,

$\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}$

where,

$P_1$ = initial pressure of $O_2$ gas = (740-22.4) torr = 717.6 torr

$P_2$ = final pressure of $O_2$ gas at STP= 760 torr

$V_1$ = initial volume of $O_2$ gas = 280 mL

$V_2$ = final volume of $O_2$ gas at STP = ?

$T_1$ = initial temperature of $O_2$ gas = $25^oC=273+25=298K$

$T_2$ = final temperature of $O_2$ gas = $0^oC=273+0=273K$

Now put all the given values in the above equation, we get:

$\frac{717.6torr\times 280mL}{298K}=\frac{760torr\times V_2}{273K}$

$V_2=242.2mL=0.2422L$

Therefore, the volume of $O_2(g)$ produced at standard conditions of temperature and pressure is 0.2422 L

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3 years ago

A student mixes a 10.0 mL sample of 1.0 M NaOH with a 10.0 mL sample of 1.0 M HCl in a polystyrene container. The temperature of

ElenaW [278]

Answer:

The experimental value of ΔH is -50 kJ/mol

Explanation:

Step 1: Data given

Volume of 1.0 M NaOH = 10.0 mL = 0.01 L

Volume of 1.0 M HCl = 10.0 mL = 0.01 L

Temperature before mixing = 20 °C

Final temperature = 26 °C

Specific heat of solution = 4.2 J/g°C

Density = 1g/mL

Step 2: Calculate q

q = m*c*ΔT

⇒ with m = the mass

⇒ 20.0 mL * 1g/mL = 20 grams

⇒ c = specific heat of solution = 4.2 J/g°C

⇒ ΔT = T2 -T1 = 26 -20 = 6 °C

q = 20g * 4.2 J/g°C * 6°C

q = 504 J

ΔHrxn = -q ( because it's an exothermic reaction)

ΔHrxn = -504 J

Step 3: Calculate number of moles

Moles = Molarity * volume

Moles = 1M *0.01 L = 0.01 moles

Step 4: Calculate the experimental value of ΔH

ΔHrxn = -504 / 0.01 mol = -50400 J/mol = -50.4 kJ/mol

The experimental value of ΔH is -50 kJ/mol

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3 years ago

Iron-56, Iron-54, and Iron-58 are all ____ of iron

JulijaS [17]

Answer:

in the 50 place

Explanation:

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4 years ago

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A chemical lab has isolated a metallic element from a compound. The metal

trapecia [35]

Answer:

C. 1

Explanation:

Group 1 metals are highly reactive (such as Sodium) and form 1 to 1 ratio of ions with halogens (such as chlorine, bromine etc).

This happens because group 1 element can donate 1 valence electron to fulfill their octet rule and halogens can receive 1 valence electron to fulfill their octet.

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3 years ago