Question

please answer the 7 th and 11th question
$donot \: answer \: if \: you \: dont \: knw$
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Answer 1

Explanation:

The Aufbau principle states that electrons fill lower-energy atomic orbitals before filling higher-energy ones (Aufbau is German for "building-up"). By following this rule, we can predict the electron configurations for atoms or ions

Lewis structure of CO32- (carbonate) ion

In carbonate ion, there is two oxygen atoms which has -1 charge on each of them. One of these oxygen atom take a proton (H+ ion) and form a -OH group.

Is NO2- resonance structures and NO2 resonance structures are different? Yes. They are different because total valance electrons of two molecules are different. Hence lewis structures of two molecules are different and their resonance structures are also different

hope it helps✌✌

Answer 2

Answer:

question cut gaye hai , agli bar pura question dalna ok

good night

Aufbau principle

The Aufbau principle dictates the manner in which electrons are filled in the atomic orbitals of an atom in its ground state. It states that electrons are filled into atomic orbitals in the increasing order of orbital energy level. According to the Aufbau principle, the available atomic orbitals with the lowest energy levels are occupied before those with higher energy levels.

The word ‘Aufbau’ has German roots and can be roughly translated as ‘construct’ or ‘build up’. A diagram illustrating the order in which atomic orbitals are filled is provided below. Here, ‘n’ refers to the principal quantum number and ‘l’ is the azimuthal quantum number.

The Aufbau principle can be used to understand the location of electrons in an atom and their corresponding energy levels. For example, carbon has 6 electrons and its electronic configuration is 1s² 2s² 2p²

See first image

Hund’s Rule

Aufbau principle tells us that the lowest energy orbitals get filled by electrons first. After the lower energy orbitals are filled, the electrons move on to higher energy orbitals. The problem with this rule is that it does not tell about the three 2p orbitals and the order that they will be filled in.

According to Hund’s rule:

Before the double occupation of any orbital, every orbital in the sub level is singly occupied.

For the maximization of total spin, all electrons in a single occupancy orbital have the same spin.

An electron will not pair with another electron in a half-filled orbital as it has the ability to fill all its orbitals with similar energy. Many unpaired electrons are present in atoms which are at the ground state. If two electrons come in contact they would show the same behaviour as two magnets do. The electrons first try to get as far away from each other as possible before they have to pair up.

See second image

8. Have Given :-

$\scriptsize \bold{wavelength \: of \: light (λ )} = 2 \times {10}^{ - 10}$

$\bold{E = \frac{hc}{λ} }$

here,

$h = 6.626 \times {10}^{ - 34}$

$c = 3.0 \times {10}^{8} \: m {s}^{ - 1}$

$λ = 2 \times {10}^{ - 10}$

$E = \frac{6.626 \times {10}^{ - 34 } \times 3 \times {10}^{8} }{2 \times {10}^{ - 10} }$

$E = \frac{ \cancel{6.626}\times 3 \times {10}^{ - 34 } \times {10}^{8} \times {10}^{10} }{ \cancel2 }$

$E = 3.313 \times 3 \times {10}^{ - 34 \times {10}^{18} }$

$E = 9.939 \times {10}^{ - 34 + 18}$

$E = 9.939 \times {10}^{ - 18}$

9. Have Given :-

$\bold{wave \: of \: the \: light = 5 \times {10}^{ - 2} }$

$\scriptsize \bold{The \: frequency \: of \: the \: light \: wave \: (v) \: is= \frac{1}{period} }$

$= \frac{ \cancel1}{ \cancel5 \times {10}^{ - 2} }$

$= 0.2 \times {10}^{2}$

$= 2 \times 10$

$\scriptsize\bold{The \: wavelength \: of \: light \: wave \: is = \frac{c}{v} }$

$= \frac{ \cancel3 \times {10}^{8} }{ \cancel2 \times 10}$

$= 1.5 \times {10}^{8} \times {10}^{ - 1}$

$= 1.5 \times {10}^{7}$

$= 15 \times {10}^{6} \: m$

$10 . \: \: \: CO ^{ - 2} _3 \: \: \: see \: image$

In carbonate ion, there is two oxygen atoms which has -1 charge on each of them. One of these oxygen atom take a proton (H+ ion) and form a -OH group.

$NO^{ - } _3 \: \: see \: second \: image$

$NO^{ - } _2 \: \: see \: \: third \: \: image$

See 4th and 5th image