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xxMikexx [17]
3 years ago
14

Which pair of atoms will MOST likely form a covalent bond?

Chemistry
1 answer:
Gelneren [198K]3 years ago
4 0

Answer:

An atom with 1 valence electron and an atom with 7 valence electrons

Explanation:

Covalent bond:

It is formed by the sharing of electron pair between bonded atoms.  

The atom with larger electronegativity attract the electron pair more towards it self and becomes partial negative while the other atom becomes partial positive.

For example:

In water the electronegativity of oxygen is 3.44 and hydrogen is 2.2. That's why electron pair attracted more towards oxygen, thus oxygen becomes partial negative and hydrogen becomes partial positive.

the number of valance electrons of oxygen are six and hydrogen is one that's why two hydrogen atoms are attached with one oxygen atom and complete the octet.

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Need help I don’t understand this at all need to show my work and strategy it’s stoichiometry gram to gram please help
laila [671]

Answer:

781×10¯² g of MgCl₂.

Explanation:

The balanced equation for the reaction is given below:

Mg + 2HCl —> MgCl₂ + H₂

Next, we shall determine the mass of HCl that reacted and the mass of MgCl₂ produced from the balanced equation. This is illustrated below:

Molar mass of HCl = 1 + 35.5

= 36.5 g/mol

Mass of HCl from the balanced equation = 2 × 36.5 = 73 g

Molar mass of MgCl₂ = 24 + (35.5×2)

= 24 + 71

= 95 g/mol

Mass of MgCl₂ from the balanced equation = 1 × 95 = 95 g

SUMMARY:

From the balanced equation above,

73 g of HCl reacted to produce 95 g of MgCl₂.

Finally, we shall determine the mass of MgCl₂ produced by the reaction of 6 g of HCl. This can be obtained as follow:

From the balanced equation above,

73 g of HCl reacted to produce 95 g of MgCl₂.

Therefore, 6 g of HCl will react to produce = (6 × 95)/73 = 781×10¯² g of MgCl₂.

Thus, 781×10¯² g of MgCl₂ were obtained from the reaction.

4 0
3 years ago
Using the following data, determine the standard cell potential E^o cell for the electrochemical cell constructed using the foll
Nana76 [90]

Answer: C)  0.637 V

Explanation:

The balanced redox reaction is:

Zn(s)+Pb^{2+}(aq)\rightarrow Zn^{2+}(aq)+Pb(s)

Here Zn undergoes oxidation by loss of electrons, thus act as anode. Lead undergoes reduction by gain of electrons and thus act as cathode.

E^0=E^0_{cathode}- E^0_{anode}

Where both E^0 are standard reduction potentials.

Zn^{2+}(aq)+2e^-\rightarrow Zn(s)= -0.763

Pb^{2+}(aq)+2e^-\rightarrow Pb(s)= -0.126

E^0_{[Zn^{2+}/Zn]}=-0.763V

E^0_{[Pb^{2+}/Pb]}=-0.126V

E^0=E^0_{[Pb^{2+}/Pb]}- E^0_{[Zn^{2+}/Zn]}

E^0=-0.126-(-0.763V)=0.637V

The standard emf of a cell is 0.637 V

8 0
3 years ago
At what temperature does a gas at 1.00 atm and 20 degree Celsius have a pressure of 4.00 atm.
vfiekz [6]

Answer:

P1 =4 atm

T1= 20°C

P2=1 atm

T2=?

According to Gay-Lussac's Law or Third Gas Law,

P1T2=P2T1

4×T2=1×20

T2= 20/4

T2= 5°C

Answer At 5°C temperature does a gas at 1.00 atm !

7 0
3 years ago
Magnesium has three naturally occurring isotopes, ²⁴Mg (isotopic mass = 23.9850 amu, abundance = 78.99%), ²⁵Mg (isotopic mass =
joja [24]

The atomic mass of the  magnesium is : 24.31⋅g.

<h3>What is isotopes?</h3>

Isotopes are members of a family of elements that all have the same number of protons and different numbers of neutrons. The number of protons in the nucleus determines the atomic number of an element on the periodic table.

Magnesium has three natural isotopes: ²⁴Mg, ²⁵Mg, and ²⁶Mg.

<h3>What is atomic mass ?</h3>

Atomic mass is the mass of an atom. The SI unit of mass is the kilogram, while atomic mass is often expressed in the non-SI unit dalton (synonymous with uniform atomic mass unit). 1 Da is defined as 1/12 the mass of a free carbon-12 atom at rest in the ground state.

Calculation :

The atomic mass is the weighted average of the individual isotopic masses:

(23.99×78.99%+24.99×10.00%+25.98×11.01%)⋅g=24.31⋅g

To know more atomic mass please click here : brainly.com/question/338808

#SPJ4

4 0
1 year ago
A planetary explorer vehicle
lana66690 [7]

Answer:

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Explanation:

6 0
3 years ago
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