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-BARSIC- [3]
2 years ago
14

Which of the following corresponds to an alpha particle?

Chemistry
1 answer:
andrey2020 [161]2 years ago
4 0

Answer:

Atomic number=No. of protons=No. of electrons in ground state(unchanged atom)

Atomic number=13=No. of protons

Atomic mass=no. of protons+no. of neutrons=13+14=27

For isotope no. of proton=13(same atomic number but different mass number are isotopes)

no. of electrons=13

no. of neutrons=14+2=16

Explanation:

hope it's help you

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Hydrogen sulfide,H2S, is a very toxic gas with a smell of rotten eggs. using the following: H2S+3/2 O2=SO2+H2O H2+1/2O2=H2O S+O2
Serga [27]

Answer:

ΔH = -20kJ

Explanation:

The enthalpy of formation of a compound is defined as the change of enthalpy during the formation of 1 mole of the substance from its constituent elements. For H₂S(g) the reaction that describes this process is:

H₂(g) + S(g) → H₂S(g)

Using Hess's law, it is possible to sum the enthalpies of several reactions to obtain the change in enthalpy of a particular reaction thus:

<em>(1) </em>H₂S(g) + ³/₂O₂(g) → SO₂(g) + H₂O(g) ΔH = -519 kJ

<em>(2) </em>H₂(g) + ¹/₂O₂(g) → H₂O(g) ΔH = -242 kJ

<em>(3) </em>S(g) + O₂(g) → SO₂(g) ΔH = -297 kJ

The sum of -(1) + (2) + (3) gives:

<em>-(1) </em>SO₂(g) + H₂O(g) → H₂S(g) + ³/₂O₂(g) ΔH = +519 kJ

<em>(2) </em>H₂(g) + ¹/₂O₂(g) → H₂O(g) ΔH = -242 kJ

<em>(3) </em>S(g) + O₂(g) → SO₂(g) ΔH = -297 kJ

<em>-(1) + (2) + (3): </em><em>H₂(g) + S(g) → H₂S(g) </em>

<em>ΔH =</em> +519kJ - 242kJ - 297kJ = <em>-20 kJ</em>

<em />

I hope it helps!

5 0
2 years ago
Which is the strongest acid? Ch3ch2ch2chfch2co2h ch3ch2ch2cbr2ch2co2h ch3ch2ch2cf2ch2co2h ch3chbrch2ch2ch2co2h ch2clch2ch2ch2ch2
liq [111]

The strength of an acid increases if the stability of conjugate base increases

The stability of a conjugate base increases with the presence of electron with drawing group (electronegative group)

Thus more the electronegativity of an atom attached to a carboxylic acid higher the strength of acid

In these examples CH3CH2CH2CF2CH2COOH contains to electronegative flourine atoms which stabilizes the conjugate base hence this will be the strongest acid among the given acids

8 0
3 years ago
Write the ionic charges (such as Ca2+) and chemical formulas and fill-in the table below.
Vikentia [17]

1) Lithium and fluorine:

Ionic charges: lithium cation Li⁺ and fluorine anion F⁻.

Chemical formula LiF.

In ionic salt lithium fluoride (LiF), fluorine has electronegativity approximately χ = 4 and lithium χ = 1 (Δχ = 4 - 1; Δχ = 3).

Fluorine attracts electron and it has negative charge and lithium has positive charge.

2) Beryllium and oxygen:

Ionic charges cation Be²⁺ and anion O²⁻.

Chemical formula is BeO.

Beryllium is metal from group 2 and oxygen is nonmetal from group 16.

Electron configuration of beryllium: ₄Be: 1s² 2s², it has two valence electrons in 2s orbital.

Beryllium lose two electrons and to gain electron configuration as noble gas helium (He).

Electron configuration of oxygen atom: ₈O 1s² 2s² 2p⁴.

Oxygen gain two valence electron to form anion with stable electron configuration as noble gas neon (atomic number 10).

3) Magnesium and fluorine:  

Ionic charges cation Mg²⁺ and anion F⁻.

Chemical formula is MgF₂.

Magnesium fluoride (MgF₂) is salt, ionic compound.  

Magnesium (Mg) is metal from 2. group of Periodic table of elements and has low ionisation energy and electronegativity, which means it easily lose valence electons (two valence electrons).  

Magnesium has atomic number 12, which means it has 12 protons and 12 electrons. It lost two electrons to form magnesium cation (Mg²⁺) with stable electron configuration like closest noble gas neon (Ne) with 10 electrons.  

Fluorine (F) is nonmetal with greatest electronegativity, which means it easily gain electrons.  

Fluorine has atomic number 9, which means it has 9 protons and 9 electrons. It gain one electron to form fluorine anion (F⁻) with stable electron configuration like closest noble gas neon (Ne) with 10 electrons.  

4) Aluminum and chlorine:  

Ionic charges cation Al³⁺ and anion Cl⁻.

Chemical formula is AlCl₃.

The right name for AlCl₃ is aluminium chloride.

Aluminium chloride is a salt with ionic bonds.

Aluminium (metal from group 13) has oxidation number +3 and chlorine (nonmetal from group 17) has oxidation number -1, chemical compound has neutral charge (+3 + 3 · (-1) = 0).

5) Beryllium and nitrogen:  

Ionic charges cation Be²⁺ and anion N³⁻.

Chemical formula is Be₃N₂.

Atomic number of nitrogen is 7, it has 7 protons and 7 electrons.

Electron configuration of nitrogen atom: ₇N 1s² 2s² 2p³.

Nitrogen gain three electrons to form anion with stable electron configuration as noble gas neon (atomic number 10).

4 0
2 years ago
What is the mass of HCL is consumed by the reaction of 1.5 mole of magnesium
photoshop1234 [79]

Answer: 109.5g

Explanation:

Mg + 2HCl —> MgCl2 + H2

From the equation,

1mole of Mg required 2moles of HCl

Therefore 1.5moles of Mg will require = 1.5 x 2 = 3 moles of HCl.

Molar Mass of HCl = 1+35.5 =36.5g/mol

Mass conc. Of HCl = 3 x 36.5 = 109.5g

3 0
2 years ago
Naturally occurring neon exists as three isotopes. 90.51% is ne-20 with a mass of 19.99 amu, 0.27% is ne-21 with a mass of 20.99
gregori [183]

The atomic mass of an element is the average relative mass of its atoms as compared with an atom of carbon-12 whose mass is taken as 12. In terms of percentages of different isotopes, the average atomic mass can be determined as follows: A_{average} = ∑(p_{i}X A_{i})/100. Where, p_{i} is the percentage abundance of isotope with atomic number A_{i}.

So, average atomic mass of neon = \frac{(90.51 X 19.99) + (0.27 X 20.99) + (9.22 X 21.99)}{100} = 20.177 amu.

3 0
3 years ago
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