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Katyanochek1 [597]
3 years ago
12

Review the families and classification of elements in the periodic table. Based on this information, you would expect elements t

o the left of the stair-step line in the periodic table to form ________ ions and have __________ valence electron(s).
A) positive; 1
B) negative; 4 - 7
C) positive; four or less
D) negative; three or less
Chemistry
2 answers:
AlekseyPX3 years ago
8 0

Answer:

A.

Explanation:

They lose 1 electrons in their outermost shell.

The proton to electron ratio become unbalanced where the proton overpowers.

Therefore, leaving the ion positively charged.

inn [45]3 years ago
6 0
It is b because I need to answer my first question
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What type of bond would be found between
LenaWriter [7]

Answer:

  1. covalent bond
  2. polar covalent bond
  3. ionic bond
  4. metallic bond

Explanation:

<h2>hope it helps you </h2><h2>.</h2><h2>.</h2><h2>.</h2><h2>.</h2><h2>.</h2><h2>.</h2><h2>Thank uu</h2>
3 0
3 years ago
You are given a solid that is a mixture of Na2SO4 and K2SO4. A 0.205-g sample of the mixture is dissolved in water. An excess of
Svetach [21]

Answer:

Mass of SO₄⁻² = 0.123 g.

Mass percentage of SO₄⁻² = 41.2%

Mass of Na₂SO₄ = 0.0773 g

Mass of K₂SO₄ = 0.1277 g

Explanation:

Here we have

We place Na₂SO₄ = X and

K₂SO₄ = Y

Therefore

X +Y = 0.205 .........(1)

Therefore since the BaSO₄ is formed from BaCl₂, Na₂SO₄ and K₂SO₄ we have

Amount of BaSO₄ from Na₂SO₄ is therefore;

X\times\frac{Molar \, Mass \, of \, BaSO_4}{Molar \, Mass \, of \, Na_2SO_4}

Amount of BaSO₄ from K₂SO₄ is;

Y\times\frac{Molar \, Mass \, of \, BaSO_4}{Molar \, Mass \, of \, K_2SO_4}

Molar mass of

BaSO₄ = 233.38 g/mol

Na₂SO₄ = 142.04 g/mol

K₂SO₄ = 174.259 g/mol

X\times\frac{Molar \, Mass \, of \, BaSO_4}{Molar \, Mass \, of \, Na_2SO_4} = X\times\frac{233.38 }{142.04} = 1.643·X

Y\times\frac{Molar \, Mass \, of \, BaSO_4}{Molar \, Mass \, of \, K_2SO_4} = Y\times\frac{233.38 }{174.259 } = 1.339·Y

Therefore, we have

1.643·X + 1.339·Y = 0.298 g.....(2)

Solving equations (1) and (2) gives

The mass of SO₄⁻² in the sample is given by

Mass of sample = 0.298

Molar mass of BaSO₄ = 233.38 g/mol

Mass of Ba = 137.327 g/mol

∴ Mass of SO₄ = 233.38 g - 137.327 g = 96.05 g

Mass fraction of SO₄⁻² in BaSO₄ = 96.05 g/233.38 g = 0.412

Mass of SO₄⁻² in the sample is 0.412×0.298 = 0.123 g.

Percentage mass of SO₄⁻² = 41.2%

Solving equations (1) and (2) gives

X = 0.0773 g and Y = 0.1277 g.

8 0
3 years ago
Combustion of ethylene glycol leads to a change in internal energy (\DeltaU) of –1189 kJ at 298 K. What is the corresponding cha
ddd [48]

Answer:

-1190.24 kJ

Explanation:

The enthalpy change in a chemical reaction that produces or consumes  gases is given by the expression:

ΔH = ΔU + Δngas RT

where  Δn gas is the change of moles of gas, R is the gas constant,and T is temperature.

Now from the given   balanced chemical reaction, the change in number of mol gas is equal to:

Δn gas = mole gas products - mole gas reactants =  2 - 5/2 = -1/2 mol

Sionce we know ΔU and the temperature (298 K), we are in position to calculate the change in enthalpy.

ΔH = -1189 x 10³ J + (-0.5 mol ) 8.314 J/Kmol x 298 K

ΔH = -1.190 x 10⁶ J = -1.190 x 10⁶ J x 1 kJ/1000 J = -1.190 x 10³ J

7 0
3 years ago
How many moles of N2 are in a flask with a volume of 0.5 L at a pressure of 400.0 kPa and a temperature of 300.0 K?
mylen [45]

Answer:

0.08moles

Explanation:

Given parameters:

Volume of gas  = 0.5L

Pressure of gas  = 400kPa

Temperature of gas  = 300K

Unknown:

Number of moles of N₂ = ?

Solution:

Applying the ideal gas law which is a combination of the three gas law: Boyle's law, Charles's law and Avogadro's law will solve this problem.

The ideal gas law is stated as;

              PV  = nRT

P is the pressure of the gas

V is the volume of the gas

n is the number of moles

R is the gas constant

T is the temperature of the gas

  We need to convert kPa of the pressure to atm which is a more comfortable unit to work with.

      400kPa will be \frac{400}{101.325}   = 3.95atm

Input the variables in the equation;

             3.95 x 0.5  = n x 0.082 x 300

                            n  = 0.08moles

5 0
3 years ago
The density of a metal is 9.80 g/mL. What is the mass of a sample of metal when dropped in 28.9 mL of water, the volume increase
yan [13]

The correct answer is 2.70 × 10² g or 270 g.  

It is given, that the density of a metal is 9.80 g/ml.  

Let the mass of a sample of metal be x.  

The sample of metal is dropped in 28.9 ml of water, due to which the volume of the water increases to 56.4 ml.  

In order to calculate the mass of a metal, there is a need to use the formula, mass = density * volume

Mass = (9.80 g/ml) (56.4 ml - 28.9 ml)

= (9.80 g/ml) (27.5 ml)

= 2.70 × 10² g or 270 g


6 0
3 years ago
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