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topjm [15]
3 years ago
12

When atoms from Column I (Group 1) combine with atoms from Column VII (Group 17): A nearly 100% covalent bond forms. The bond wi

ll be ionic. A weak bond will form. The resulting compound will be very unstable. A great deal of energy is absorbed.
Chemistry
2 answers:
gtnhenbr [62]3 years ago
7 0

The answer you're looking for is B. The bond will be ionic.

kotykmax [81]3 years ago
6 0

Answer:

When atoms from Column I (Group 1) combine with atoms from Column VII (Group 17) <u><em>the bond will be ionic.</em></u>

Explanation:

An ionic bond is produced between metallic and non-metallic atoms, where electrons are completely transferred from one atom to another. During this process, one atom loses electrons and another one gains them, forming ions. Usually, the metal gives up its electrons forming a cation to the nonmetal element, which forms an anion.

In other words, by forming ionic compounds, the elements to the left of the periodic table usually lose electrons, and form a cation that has the same electronic configuration as the nearest noble gas. The elements to the right of the periodic table tend to gain electrons to reach the electronic configuration of the next noble gas .

This type of bond is produced by the attraction of ions with opposite charges. By assigning or accepting the valence electrons, the ions comply with the octet rule and are more stable. Remember that valence electrons are the electrons of the outermost layer of the atom, which can participate in chemical bonds.

It is also possible to think that an ionic bond is formed when two atoms have a very large electronegativity difference, remembering that electronegativity is the property of an atom to attract an electron.  And this large difference in electronegativity usually occurs between the atoms of Column I (Group 1) combined with atoms of Column VII (Group 17).

Then it is finally possible to say that <u><em>"When atoms from Column I (Group 1) combine with atoms from Column VII (Group 17) the bond will be ionic."</em></u>

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rjkz [21]

Explanation:

Let us assume that the concentration of [OH^{-} and H^{+} is equal to x. Then expression for K_{w} for the given reaction is as follows.

          K_{w} = [OH^{-}][H^{+}]

          K_{w} = x^{2}

      6.8 \times 10^{-15} = x^{2}

Now, we will take square root on both the sides as follows.

          \sqrt{6.8 \times 10^{-15}} = \sqrt{x^{2}}

          [H^{+}] = 8.2 \times 10^{-8} M

Thus, we can conclude that the H_{3}O^{+} concentration in neutral water at this temperature is 8.2 \times 10^{-8} M.

8 0
3 years ago
Read 2 more answers
How many grams of Co are needed to react with an excess of fe203 to produce 156.2 g FE? show your work.
Gekata [30.6K]

The reaction is given as

Fe2O3 (s)+ 3CO(g)--->3CO2(g)+ 2Fe(s)

No.of moles=mass in gram/molar mass

As for Fe mole =156.2g/55.847=2.7969~2.797

The ratio b/w CO and Fe is 3:2

Moles of CO needed= 2.797x3/2=4.1955

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8 0
3 years ago
Which of these is the smallest volume 500mL, 2,500 cm3, 5.5•10-1, 25 m3
mezya [45]
25m³.
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3 years ago
2 FONS
stiv31 [10]

Answer:

C. It decreases by a factor of 4

Explanation:

F1 = kq1*q2/r²

F2 = kq1*q2/(2r)² = kq1*q2/(4r²) = kq1*q2/(r²*4)  = F1/4

7 0
2 years ago
What is the volume of 2 mol of chlorine gas at STP?<br> 2.0 L<br> 11.2 L<br> 22.4 L<br> 44.8 L
nirvana33 [79]

Answer:

44.8 L

Explanation:

Using the ideal gas law equation:

PV = nRT

Where;

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V = volume (L)

n = number of moles (mol)

R = gas law constant (0.0821 Latm/molK)

T = temperature (K)

At Standard temperature and pressure (STP);

P = 1 atm

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Hence, when n = 2moles, the volume of the gas is:

Using PV = nRT

1 × V = 2 × 0.0821 × 273

V = 44.83

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2 years ago
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