CHEMISTRY COLLEGE

Which of the following electron configurations represents an excited state of the indicated atom? Group of answer choices a.Na: 1s2 2s2 2p6 3s2 3p2 3s1
b.Ne: 1s2 2s2 2p6
c.N: 1s2 2s2 2p3
d.P: 1s2 2s2 2p6 3s2 3p2 4s1
e.He: 1s2

Answers

Answer 1

Answer:

Answer: The electronic configuration of the atom that represents excited state is P: $1s^22s^22p^63s^23p^24s^1$

Explanation:

There are 2 states classified under energy levels:

Ground state: This is the lower energy state which is termed as stable state.
Excited state: This is the upper energy state and is termed as the unstable state. All the electrons which are present in this state always come back to the ground state.

For the given options:

For a: Sodium

The atomic number of sodium element is 11. The ground state electronic configuration of this element is $1s^22s^22p^63s^1$

For b: Neon

The atomic number of neon element is 10. The ground state electronic configuration of this element is $1s^22s^22p^6$

For c: Nitrogen

The atomic number of nitrogen element is 7. The ground state electronic configuration of this element is $1s^22s^22p^3$

For d: Phosphorus

The atomic number of phosphorus element is 15. The ground state electronic configuration of this element is $1s^22s^22p^63s^23p^3$

One electron from the valence shell jumps into outer shell and the excited state electronic configuration becomes $1s^22s^22p^63s^23p^24s^1$

For e: Helium

The atomic number of helium element is 2. The ground state electronic configuration of this element is $1s^2$

Hence, the electronic configuration of the atom that represents excited state is P: $1s^22s^22p^63s^23p^24s^1$

Answer 2

Answer:

Final answer:

The sodium atom with the electron configuration 1s2 2s2 2p6 3s2 3p2 3s1 is in an excited state because other sodium atom stages are not completely filled.

Explanation:

An atom is in an excited state when one or more electrons have moved to a higher energy level. Normal electron configurations have the electrons in the lowest possible energy states (or orbitals). In this case, the answer choice is (a) sodium (Na) with the electron configuration 1s2 2s2 2p6 3s2 3p2 3s1. Sodium normally has the 3s state fully occupied, so the presence of an electron in a higher energy state (3p) and the vacancy in the lower energy state (3s) indicates an excited state.

Learn more about Excited State here:

brainly.com/question/32724738

#SPJ3

Related Questions

The following data were obtained in a kinetics study of the hypothetical reaction A + B + C → products. [A]0 (M) [B]0 (M) [C]0 (M) Initial Rate (10–3 M/s) 0.4 0.4 0.2 160 0.2 0.4 0.4 80 0.6 0.1 0.2 15 0.2 0.1 0.2 5 0.2 0.2 0.4 20 Using the initial-rate method, what is the order of the reaction with respect to C? a. zero-order b. first-order c. third-order d. second-order e. impossible to tell from the data given
How many atoms are in 2.3 moles Au?
A sample containing only carbon, hydrogen, and silicon is subjected to elemental analysis. After complete combustion, a 0.7020 g sample of the compound yields 1.4 g of CO2, 0.86 g of H2O, and 0.478 g of SiO2. What is the empirical formula of the compound?
Unknown A melts at 113- 114oC. Known compounds 3-Nitroaniline and 4-Nitrophenol both melt at 112-114 oC. If A is mixed with 3-Nitroaniline and the melting point becomes broad and depressed, what must A be __________A) 3-Nitroaniline B) 4-Nitrophenol C) Both
Isn't this false? For the industrial production of indigo carmine, a blue food colouring additive, a synthetic process with an E-factor of 17.4 produces less waste than a synthetic process with an E-factor of 3.0. The answer I got was False, is this correct?

What is the total mass (amu) of carbon in each of the following molecules?(a)CH4
(b)CHCL3
(c)C12H10O16
(d)CH3CH2CH2CH2CH3

Answers

The mass of carbon in $\rm CH_4$ is 12.007 amu, $\rm CHCl_3$ is 12.007, $\rm C_1_2H_1_0O_1_6$ is 144.084 amu, and $\rm CH_3CH_2CH_2CH_2CH_3$ is 60.035 amu.

What is the mass of one Carbon atom?

The mass has been given as the sum of the atomic mass unit in the compound. The mass of 1 atom of carbon is 12.007 amu.

The mass of carbon in the following compounds is given as:

$\rm CH_4$

The number of Carbon units = 1

The mass of carbon in compound = 12.007 amu

$\rm CHCl_3$

The number of Carbon units = 1

The mass of carbon in the compound = 12.007 amu

$\rm C_1_2H_1_0O_1_6$

The number of carbon units =12

The mass of carbon in the compound:

$\rm 12\;*\;12.007\;amu\n=144.084\;amu$

$\rm CH_3CH_2CH_2CH_2CH_3$

The number of carbon units = 5

The mass of carbon in the compound:

$\rm 5\;*\;12.007\;amu\n=60.035\;amu$

Learn more about the mass of an atom, here:

brainly.com/question/5566317

Answer:

The atomic mass of carbon (C) is 12.0107 amu, so if you want to calculate the total mass in each molecule, you just need to multiply the number of carbon atoms in the substance by 12.017. In (a) there is one atom of C, (b) have also one atom of C, (c) have 12 atoms of C, and (d) have five atoms of C. Thus, the total mass (amu) of carbon is:

(a) 12.017 amu

(b) 12.017 amu

(d) 60.085 amu

Suppose that you are a scientist who studies climate changes. While examining the rings of tree trunks, you notice several very large tree rings. What can you conclude about the climate during those years?

Answers

Answer:

The climate was wet and cold

Explanation:

Answer:

The large tree rings allow you to conclude that the climate was either very warm or wet during those growing seasons, because greater than normal growth occurred.

Explanation: It is the edge sample response

What is the mass, in grams, of 1.20×1021 molecules of aspirin, c9h8o4?

Answers

Answer: The mass of given number of molecules of aspirin is 0.359 grams.

Explanation:

We are given:

Number of molecules of aspirin = $1.20* 10^(21)$

We know that:

Molar mass of aspirin $(C_9H_8O_4)$ = 180.16 g/mol

According to mole concept:

$6.022* 10^(23)$ number of molecules are contained in 1 mole of a compound

Also, $6.022* 10^(23)$ number of molecules of aspirin has a mass of 180.16 grams

So, $1.20* 10^(21)$ number of molecules will have a mass of $(180.16)/(6.022* 10^(23))* 1.20* 10^(21)=0.359g$

Hence, the mass of given number of molecules of aspirin is 0.359 grams.

The mass in grams of 1.20 x10^21 molecules of asprin is 0.359 grams

calculation

find the number of moles of aspirin by use of Avogadro's law that is 1 mole =6.02 x10^23 molecules

what of 1 .20 x10^21 molecules

= (1 mole x 1.20 x10 ^21 molecules)/6.02 x10^23 molecules)= 1.993 x10^-3 moles

mass of aspirin= moles x molar mass

molar mass of aspirin = (12 x9)+(1 x8) +(16x4)=180 g/mol

mass= 1.993 x10^-3 moles x180 g/mol = 0.359 grams

Isopropyl methyl ether is slightly soluble with water because the oxygen atom of ethers with three or fewer carbon atoms can form a few hydrogen bonds with water.(A) True
(B) False

Answers

Isopropyl methyl ether is slightly soluble in water because the oxygen atom of ethers with 3 or lesser carbon atoms can form hydrogen bonds with water. Therefore, the given statement is true.

What is hydrogen bonding?

Hydrogen bonding is a special class of attractive intermolecular forces that arise because of the dipole-dipole interaction between hydrogen that is bonded to a highly electronegative atom and another highly electronegative atom that lies in the neighborhood of the hydrogen atom.

For example, in water, hydrogen is covalently bonded to the oxygen atom. Therefore, hydrogen bonding arises because of the dipole-dipole interactions between the hydrogen atom of one water molecule and the oxygen atom of another water molecule.

The solubility of ether in water depends upon the extent of the formation of hydrogen bonds with water. Ether which contains three carbon atoms is soluble in water due to these lower hydrocarbon atoms can form hydrogen bonding with water.

But the solubility of hydrocarbons or ethers decreases as increase the number of carbon atoms. This is because higher ethers or ethers with more carbons have more hydrophobic parts. Therefore they cannot be soluble in water as they cannot form hydrogen bonds with water molecules.

Learn more about hydrogen bonding, here:

brainly.com/question/15099999

#SPJ2

Answer:

True

Hydrogen bond is a partial intermolecular bonding interaction between a lone pair on an electron rich donor atom, particularly the second-row elements nitrogen (N), oxygen (O), or fluorine (F), and the antibonding orbital of a bond between hydrogen (H) and a more

electronegative atom or group. Such an interacting system is generally denoted Dn–H···Ac, where the solid line denotes a polar covalent bond, and the dotted or dashed line indicates the hydrogen bond. The use of three centered dots for the hydrogen bond is specifically recommended by the IUPAC. While hydrogen bonding has both covalence and electrostatic contributions, and the degrees to which they contribute are currently debated, the present evidence strongly implies that the primary contribution is covelant.

Hydrogen bonds can be intermolecular (occurring between separate molecules) or

intramolecular (occurring among parts of the same molecule)

What volume in milliliters of H20 you need during preparation of 100 milliliters of 14.00 M H2SO4 solution starting with bottle of 17.5 M H2SO4? (Round your answer to closest integer)

Answers

Answer:

20 mL

Explanation:

We can determine the required volume of the concentrated (17.5 M) H₂SO₄ solution by using the C₁V₁=C₂V₂ formula:

17.5 M * V₁ = 14.00 M* 100 mL

V₁ = 80 mL

As out of the 100 mL of the final solution, 80 mL are from the concentrated H₂SO₄ solution, the remaining 20 mL are of water (H₂O).

What is the molarity of a solution prepared from 25.0 grams of methanol (CH3OH, density = 0.792 g/mL) with 100.0 milliliters of ethanol (CH3CH2OH)? Assume the volumes are additive.

Answers

Final answer:

The molarity of a solution prepared from 25.0 grams of methanol and 100.0 milliliters of ethanol is approximately 7.80 M.

Explanation:

This is a question about calculating molarity, which is a measure of concentration using moles per liter. To calculate the molarity of a methanol in ethanol, we first have to convert the mass of methanol into moles. The molar mass of methanol (CH3OH) is about 32.04 g/mol. Therefore, 25.0 g of methanol equals about 0.780 moles (25.0 g ÷ 32.04 g/mol).

Next, the volume of ethanol needs to be converted from milliliters to liters. Thus, 100.0 mL becomes 0.100 L. Finally, the molarity is calculated by dividing the moles of methanol by the volume of the ethanol in liters, resulting in a molarity of approximately 7.80 M (0.780 moles ÷ 0.100 L).