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3 years ago

Plz help me with the electron dot structures! I’ll mark brainliest!

Chemistry

1 answer:

diamong [38]3 years ago

8 0

The electron dot structure for each molecule are:
.. ..
a. H:O:O:H
.. ..
The partial negative charges are on the Oxygen atoms.

..
b. H:Cl:
..
The partial negative charge is on the Chlorine atom.

..
c. H:Br:
..
The partial negative sign is on Bromine atom.

..
d. H:O:H
..
The partial negative sign is on the Oxygen atom.

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What would the expected temperature change be (in Fahrenheit) ida 0.5 gran sample of water released 50.1 J of heat energy? The s

Mariana [72]

<h3>Answer:</h3>

23.95 °C

<h3>Explanation:</h3>

We are given;

Mass of the sample is 0.5 gram
Quantity of heat released as 50.1 Joules
Specific heat capacity is 4.184 J/g°C

We are required to calculate the change in temperature;

Quantity of heat absorbed is given by the formula;

Q = mass × specific heat capacity × Change in temperature

That is, Q = mcΔT

Rearranging the formula;

ΔT = Q ÷ mc

Therefore;

ΔT = 50.1 J ÷ (0.5 g × 4.184 J/g°C)

= 23.95 °C

Therefore, the expected change in temperature is 23.95 °C

4 0

4 years ago

Stoichiometry Problems!

lisov135 [29]

Hey there!

C₆H₁₂O₆(s) + 6O₂(g) => 6CO₂(g) + 6H₂0(l)

a.)

First we need to find how many molecules of oxygen gas we need.

Every one molecule of C₆H₁₂O₆ will react with six molecules of O₂. So, if we have 3.011 x 10²³ molecules of C₆H₁₂O₆, we need six times that of oxygen.

3.011 x 10²³ x 6 = 18.066 x 10²³ = 1.8066 x 10²⁴

So we need 1.8066 x 10²⁴ molecules of O₂. We need to find the volume of this in liters.

At STP, one mole of a gas occupies 22.4 liters. Let's find the number of moles we have of O₂.

(1.8066 x 10²⁴) ÷ (6.022 x 10²³) = 3 moles

3 x 22.4 = 67.2

67.2 liters of O₂ is needed.

b.)

Okay, so to find the percent yield, we need to find the theoretical yield and the actual yield. We are given the actual yield, so what we need is the theoretical yield.

For every one mole of C₆H₁₂O₆, theoretically 6 moles of H₂O will be produced.

Let's convert grams to moles for C₆H₁₂O₆:

1 gram / 180 grams = 0.0055556 moles C₆H₁₂O₆

Theoretically, 6 times that is the moles of H₂O produced:

0.0055556 x 6 = 0.033333 moles H₂O

Molar mass of H₂O is 18.015, so let's find grams:

0.033333 x 18.015 = 0.600 grams H₂O

So we have our theoretical yield, 0.600, and our actual yield, 0.303.

0.303 ÷ 0.600 = 0.505

Convert to a percent: 0.505 x 100 = 50.5%

The percent yield is 50.5%.

Hope this helps!

4 0

3 years ago

When 18.9 kJ is transferred to a gas sample in a constant volume adiabatic container with a calorimeter constant of 2.22 Kj/K, t

poizon [28]

Answer:

(a) Cgas = 0.125 kJ/k

(b) cgas = 0.25kJ/kg.K

Explanation:

18.9 kJ is equal to the sum of the heat absorbed by the gas and the heat absorbed by the calorimeter.

Qcal + Qgas = 18.9 kJ [1]

We can calculate the heat absorbed using the following expression.

Q = C . ΔT

where,

C is the heat capacity

ΔT is the change in the temperature

<em>(a) What is the heat capacity of the sample?</em>

From [1],

Ccal . ΔT + Cgas . ΔT = 18.9 kJ

(2.22kJ/K) × 8.06 K + Cgas × 8.06 K = 18.9 kJ

Cgas = 0.125 kJ/k

<em>(b) If the sample has a mass of 0.5 kilograms, what is the specific heat capacity of the substance?</em>

We can calculate the specific heat capacity (c) using the following expression:

$c=\frac{C}{m} =\frac{0.125kJ/K}{0.5kg} =0.25kJ/kg.K$

<em>(c) If the sample is Krypton, what is the molar heat capacity at constant volume of Krypton? The molar mass of Krypton is 83.8 grams/mole.</em>

The molar heat capacity is:

$\frac{0.25kJ}{kg.K} .\frac{1kg}{1000g} .\frac{83.8g}{mol} =0.021kJ/mol.K$

3 0

3 years ago

Temperature, density, and pressure ______________ (increases, decreases) as depth ____________ (increases, decreases).

Alisiya [41]

Answer:

increase/increase

Explanation:

4 0

3 years ago

Read 2 more answers

How can ionic bonds and naming be used in a real life example ?

Stells [14]

Answer:

Melting snow more efficiently in winters, understanding the components of mineral water

Explanation:

Let's split this question into two parts. First of all, ionic bonds:

an example would be the application of the freezing point depression law. Remember that adding a solute to a specific solvent would decrease the freezing point of a solvent. This is the reason why we add ionic salts, NaCl, to snow in order to make it melt. Knowledge of the fact that 1 mol of NaCl, an ionic compound, dissociates into 2 mol of ions, sodium and chloride, yields us a van 't Hoff factor of 2 rather than 1 for non-electrolytes, molecular compounds. This means the same molality of ionic compounds would produce a twice larger decrease in the freezing point of a solvent;
an example for ionic naming is more trivial. Remember the difference between, say, calcium and calcium cation. Sometimes we may read that mineral water is full of calcium. Having chemical knowledge of ionic compound naming would lead us to a conclusion that this is wrong! Mineral water doesn't have any calcium in it, we don't see any metal in mineral water. However, mineral water contains calcium cations, $Ca^{2+}$ and not $Ca$ .

8 0

3 years ago