Generate Quiz 6A91D62D7FBC9

In order to determine that the particles in the beam were negatively charged, Thomson was able to divert the cathode ray in the direction of a positively charged plate. Thomson then measured the amount that the particles were bent by different magnetic field strengths. Thomson calculated an electron’s mass to charge ratio using this information.

Since J.J. Thomson did not discover any of the other options, they are all incorrect.

The mass of water is 18g (16+2). Thus, 0.5 mol is equal to 9g of ice (H2O). Since 1 mol contains 6.02×1023 molecules, 0.5 mol will contain 3.01×1023 molecules.

Since it is numerical, there is only one possible response.

Option D is the right one. This is so because Be is a member of Group IIA and Li is a member of Group IA. Be is smaller than Li because, as we know, the atomic radius decreases with time.

In the ground state = n = 1, hydrogen has radius = r = 0.529Å.
When n = 2 and the hydrogen is excited,

as r = 0.529(n²) Å.
The radius of hydrogen in its excited state is therefore four times larger than Bohr’s radius, or r = 0.529(22Å) = 0.529(4) Å.

Mass of 1 mole of H2 = 2×1= 2g

Mass of 1 mole of Cl2 = 2×35.5 = 71g

2: 71

1: 35.5

Since (a) C3H4O3 matches the empirical formula obtained from the provided percentages of carbon, hydrogen, and oxygen, it is the right choice.

Excitation is the process by which an electron absorbs energy and moves from a lower energy level to a higher energy level. De-excitation is the process by which energy is released when an electron moves from a higher energy state to a lower state. An electron’s ground state is its lowest or resting energy state. The excited state of an electron is any energy level above its ground state.

According to the model, atoms’ electrons orbit in circles around their central nucleus.

B is the right choice.

The solution is smaller and quicker. Bohr’s theory states that an atom’s electron speed is inversely proportional to its orbital radius. This indicates that the electron’s speed increases as the orbit’s radius decreases.

The electron is limited by the nucleus’ electromagnetic force, which explains this. The force is stronger and the electron must move more quickly to maintain orbit when it is nearer the nucleus.

An electron’s energy level is also correlated with its orbital radius. The electron must move more quickly and with a smaller radius at lower energy levels.

With an atomic number of 20, calcium has twenty electrons. The calcium atom has two electrons in its first shell, eight in its second, eight more in its third, and two in its fourth. We classify it as a group 2 element, or an alkaline earth metal, because it has two electrons in its final shell.

The de-Broglie wavelength of electrons in the third orbit is close to the radius of the first Bohr orbit, which is x:

λ=3×2πx=6 πx (n=3)

Option A is the right one.
An atom with 35 nucleons and an atomic number of 17 has two electrons with n = 2 and l = 0. The electron’s energy level is indicated by the principal quantum number (n), and the orbital’s shape is indicated by the angular momentum quantum number (l). The electron is in the second energy level, according to the value of n = 2, and the orbital is a s orbital, according to the value of l = 0. An atom with 35 nucleons and an atomic number of 17 has two electrons with n = 2, l = 0 because the s orbital in the second energy level can accommodate up to two electrons.

You’ll have to rote learn this. Learn the units and power by heart.

The planck constant has a value of 6.626 x 10^-34Js.

Electrons occupy specific energy levels or orbits around the nucleus, according to Bohr’s model of the atom. The quantum number “n,” where n = 1, 2, 3, and so forth, represents these energy levels. The average distance between the electron and the nucleus, or the radius of the Bohr atom, is correlated with the quantum number “n.”

According to Bohr’s model, the square of the quantum number directly correlates with the electron orbit’s radius. Consequently, the expression provides the Bohr atom’s radius.

r = (4πε0n²)/(me²)

where the constant factor “(4πε0)/(me²)” is used.

This indicates that the orbit’s radius grows exponentially with an increase in “n”.

Every moving object or particle, regardless of mass, has a wave-like quality, according to De Broglie’s assertion, also referred to as the De Broglie hypothesis.

Moseley’s statement, sometimes referred to as Moseley’s law, describes the correlation between an element’s atomic number and the wavelength of its distinctive X-rays.

According to the Heisenberg uncertainty principle, sometimes referred to as the uncertainty principle, it is impossible to simultaneously and arbitrarily determine certain pairs of a quantum particle’s physical properties, such as its position and momentum.

A Danish physicist named Niels Bohr made significant advances in the theory of atoms.

Because P-3, Si-4, and S-2 are isoelectronic with K+, all three choices (a, b, and c) are accurate. They all share the same electron configuration (2, 8, 8) and have the same number of electrons as K+.

d) All of these is the right answer.

Atoms or ions with the same number of electrons are known as isoelectronic species. One electron has been removed from the potassium ion K+, giving it the configuration 2, 8, 8. Let’s examine each choice:

a) P-3: The normal electron count for phosphorus (P) is 15. It creates the P-3 ion, which has the configuration 2, 8, 8, 2, by gaining three electrons. With K+(2, 8, 8), this configuration is isoelectronic.

A is the right choice.

Each element’s isotope has a different number of neutrons but the same number of protons.

There are a certain number of isotopes for each element.

The number of protons in an atom’s nucleus is its atomic number.

Using the equation for an electron’s energy in the nth orbit

En=-{me-4Z2/8 ε2 h2 n2}

Z=1 for hydrogen and by entering constant values

Additionally, n=2, the second shell to which the ground state hydrogen electron has excited, is the first excited state of hydrogen.

En= (-2.178×10-18)×1/n2

The nucleus and atom’s outer electrons are less attracted to one another as a result of the inner electrons’ shielding effect. The ionization potential is lowered as a result of the outer electrons being easier to remove. Consequently, choices B and C are not appropriate.

‘Electronegativity’ is a measure of an atom’s ability to attract shared electrons to itself, and as the nucleus and outer electrons lose their attraction, electronegativity will also decrease, making Option D incorrect.