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Novay_Z [31]
3 years ago
5

How a metallic bond forms

Chemistry
1 answer:
Contact [7]3 years ago
6 0
Metallic bonds are formed by the valence electrons from the s and p orbitals of the interacting metal atoms delocalizing.
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. Nhiệt độ ban đầu của 344 g một mẫu sắt là 18,2oC. Nếu mẫu sắt này hấp thụ 2,25 kJ nhiệt lượng thì nhiệt độ cuối của mẫu sắt nà
Mrrafil [7]

Answer:

ano poh paki ult kasi hindi mahintindihan yan question mo hindi mahintindihwn

8 0
2 years ago
Read 2 more answers
Compare the change in pH with the addition of acid and base to deionized water and to a buffer.
iogann1982 [59]

Answer:

case1.

The addition of acid and base leads to a change in pH of the water when adding to deionized water due to fact that acid and bases dissociated in dissolving in water. If the H+ ion increases in the water as acid addition hikes it, it will result in decreasing the pH value. The intensity of the acid also affects the dissociation of the ions.

case2

Buffers are normally formed by weak acid and its conjugate base, and adding acid to the buffer it absorbs the H+ ions so the pH will be lower and adding base or increase of OH- conjugate base resists the pH value to increase.

5 0
3 years ago
Compare the ability to hold on to / attract electrons between metals and nonmetals.
skad [1K]

Nonmetals have the ability to attract electrons better than metals because they have a higher electron affinity or electronegativity than metals.

<h3>What is electronegativity?</h3>

Electronegativity is the tendency, or a measure of the ability, of an atom or molecule to attract electrons and thus form bonds.

An element in the periodic table with a high electronegativity will automatically have a high electron affinity.

Metals (low electronegativity) are known to lose electrons to non-metals (high electronegativity), hence, nonmetals have the ability to attract electrons better than metals because they have a higher electron affinity or electronegativity than metals.

Learn more about electronegativity at: brainly.com/question/2060520

#SPJ1

5 0
2 years ago
What is the concentration of H+ in a 2.5 M HCl solution?
Pavel [41]

Answer:

The concentration of H⁺ in a 2.5 M HCl solution is 2.5 M

Explanation:

As HCl is a strong acid and hence a strong electrolyte, it will dissociate as

HCl ⟶ H⁺ + Cl⁻

So, The concentration of H⁺ will be 2.5 M (same as HCl)

Thus, The concentration of H⁺ in a 2.5 M HCl solution is 2.5 M

<u>-TheUnknownScientist</u><u> 72</u>

6 0
3 years ago
Read 2 more answers
If 15.6 grams of copper (ii) chloride react with 20.2 grams of sodium nitrate how many grams of sodium chloride can be formed? W
olasank [31]

Answer:

- 13.56 g of sodium chloride are theoretically yielded.

- Limiting reactant is copper (II) chloride and excess reactant is sodium nitrate.

- 0.50 g of sodium nitrate remain when the reaction stops.

- 92.9 % is the percent yield.

Explanation:

Hello!

In this case, according to the question, it is possible to set up the following chemical reaction:

CuCl_2+2NaNO_3\rightarrow 2NaCl+Cu(NO_3)_2

Thus, we can first identify the limiting reactant by computing the yielded mass of sodium chloride, NaCl, by each reactant via stoichiometry:

m_{NaCl}^{by\ CuCl_2}=15.6gCuCl_2*\frac{1molCuCl_2}{134.45gCuCl_2} *\frac{2molNaCl}{1molCuCl_2} *\frac{58.44gNaCl}{1molNaCl} =13.56gNaCl\\\\m_{NaCl}^{by\ NaNO_3}=20.2gNaNO_3*\frac{1molNaNO_3}{84.99gNaNO_3} *\frac{2molNaCl}{2molNaNO_3} *\frac{58.44gNaCl}{1molNaCl} =13.89gNaCl

Thus, we infer that copper (II) chloride is the limiting reactant as it yields the fewest grams of sodium chloride product. Moreover the formed grams of this product are 13.56 g. Then, we take 13.56 g of sodium chloride to compute the consumed mass sodium nitrate as it is in excess:

m_{NaNO_3}^{by\ NaCl}=13.56gNaCl*\frac{1molNaCl}{58.44gNaCl}*\frac{2molNaNO_3}{2molNaCl} *\frac{84.99gNaNO_3}{1molNaNO_3}=19.72gNaNO_3

Therefore, the leftover of sodium nitrate is:

m_{NaNO_3}^{leftover}=20.2g-19.7g=0.5gNaNO_3

Finally, the percent yield is computed via:

Y=\frac{12.6g}{13.56g} *100\%\\\\Y=92.9\%

Best regards!

6 0
3 years ago
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