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10 days ago

What is the symbol for the isotope of 58 co that possesses 33 neutrons?

Chemistry

2 answers:

KiRa [971]10 days ago

6 0

The element with atomic number 58 is Cerium, meaning its symbol should be Ce rather than Co, which belongs to Cobalt with atomic number 27. Therefore, the notation for isotopes consists of the element's symbol accompanied by a superscript and a subscript, properly aligned. The superscript indicates the mass number.

Mass number = protons + neutrons = 58 + 33 = 91

The subscript denotes the atomic number, which is 58. This notation is illustrated in the attached image.

castortr0y [923]10 days ago

3 0

The notation for the isotope:

$\large {{{91} \atop {58}} \right Ce}$

Additional clarification

Elements found in nature exist in several forms known as isotopes.

Isotopes are atoms distinguished by having the same atomic number but differing in neutron count.

This means that isotopes share the same Proton (Atomic Number).

Atomic mass refers to the mean mass of all isotopes.

To determine an atom's mass, the standard is set against 1 atom of carbon-12, which has a mass of 12 amu.

This results in atomic mass being expressed relative to the carbon-12 atom.

$\large {\boxed {mass ~ average ~ atom ~ X ~ = ~ \frac {mass\:isotope ~ 1 + mass ~ isotope ~ 2} {number ~ whole ~ atom ~ X}}$

An atomic mass unit (amu) represents a relative mass of 1/12 the weight of a carbon-12 atom.

$\large {\boxed {Ar ~ X = \frac {mass ~ average ~ 1 ~ atom ~ X} {\frac {1} {12}. mass ~ 1 ~ atom ~ C-12}}}$

The unit 'amu' has now transitioned to simply 'u'.

For instance, carbon possesses three isotopes: ₆¹²C12, ₆¹³C, and ₆¹⁴C.

The Atomic Number (Z) specifies the number of protons in an element's atom. When the atom carries no charge, its proton count matches its electron count, allowing the atomic number to also reflect the electron count.

Thus, atomic number = proton count = electron count.

Mass Number (A) is calculated by adding the protons and neutrons together.

Mass Number (A) = Proton count + Neutron count.

This leads to the relationship between atomic and mass numbers given by:

Atomic Number (Z) = Mass Number (A) - Neutron count.

In notation for the element:

$\large {{{A} \atop {Z}} \right X}$

Information:

X = symbol for the element

A = mass number

= proton count + neutron count

Z = atomic number

= proton count = electron count in neutral atoms

The symbol for the isotope with mass number 58 and 33 neutrons:

The number 58 identifies the Atomic Number (Z) = proton count

And calculating the mass number gives us:

A = proton count + neutron count

A = 58 + 33

A = 91

The element with atomic number 58 is undoubtedly Cerium (Ce).

<pTherefore, the notation for the isotope:

$\large{\boxed{\bold{ {{{91} \atop {58}} \right Ce}}}}$

Explore further

element X

Keywords: the representation, the isotope, Ce, atomic number, mass number

Answer;

As and Sr ------- [Kr]

Be ------------- [He]

O and Mg ------- [Ne]

S and Ca ------- [Ar]

Explanation

The Be+ ion has 2 electrons, matching He. The Mg2+ and O2− ions possess 10 electrons each, like Ne.
S2− and Ca2+ ions each have 18 electrons, the same as Ar. The As3− and Sr+ ions hold 36 electrons, paralleling Kr.
Elements gain or lose electrons to reach a stable electron configuration akin to that of noble gases.
When atoms lose electrons, they form positive ions (cations), and when they gain electrons, they form negative ions (anions).

4 0

16 days ago

Read 2 more answers

A metallic object holds a charge of −4.8 × 10−6 C. What total number of electrons does this represent? (e = 1.6 × 10−19 C is the

Anarel [852]

Answer:

$n=3.0\times 10^{13}$

Explanation:

Charge of one electron = $-1.6\times 10^{-19}\ C$

The formula for calculating charge is:

$Charge=n\times q_e$

Given that: Charge = $-4.8\times 10^{-6}\ C$

$-4.8\times 10^{-6}=n\times (-1.6\times 10^{-19})$

$n=\frac{4.8\times 10^{-6}}{1.6\times 10^{-19}}=3.0\times 10^{13}$

Total electrons, n = $3.0\times 10^{13}$

5 0

13 days ago

2CH4(g)⟶C2H4(g)+2H2(g)

Alekssandra [968]

Answer: The enthalpy change for the reaction is, 201.9 kJ

Explanation:

Based on Hess’s law of constant heat summation, the energy released or absorbed in a chemical reaction stays constant, regardless of whether the process unfolds in one step or multiple steps.

This principle implies, that chemical equations can be treated analogously to algebraic expressions, allowing addition or subtraction to create the needed equation. Thus, the overall enthalpy change corresponds to the summation of the individual enthalpy changes of the reactions occurring in between.

The balanced equation for $CH_4$ appears as follows,

$2CH_4(g)\rightarrow C_2H_4(g)+2H_2(g)$ $\Delta H^o=?$

The intermediate balanced reactions are outlined as follows,

(1) $CH_4(g)+2O_2(g)\rightarrow CO_2(g)+2H_2O(l)$ $\Delta H_1=-890.3kJ$

(2) $C_2H_4(g)+H_2(g)\rightarrow C_2H_6(g)$ $\Delta H_2=-136.3kJ$

(3) $2H_2(g)+O_2(g)\rightarrow 2H_2O(l)$ $\Delta H_3=-571.6kJ$

(4) $2C_2H_6(g)+7O_2(g)\rightarrow 4CO_2(g)+6H_2O(l)$ $\Delta H_4=-3120.8kJ$

Next, we will multiply the first reaction by 2, reverse the second, and reverse and halve the third and fourth reactions before combining them. This gives us:

(1) $2CH_4(g)+4O_2(g)\rightarrow 2CO_2(g)+4H_2O(l)$ $\Delta H_1=2\times (-890.3kJ)=-1780.6kJ$