Atomic Structure and Quantum Model

Protons have a charge of +1 and a relative mass of 1, electrons have a charge of -1 and a relative mass of 1/1840, while neutrons have a charge of 0 and a relative mass of 1.

The Quantum model arranges electrons in shells defined by the principal quantum number, whereas the Bohr model is more simplistic and does not account for subshells or varying energy levels.

An orbital can hold a maximum of 2 electrons, which must have opposite spins: one spin up (↑) and one spin down (↓).

<p>The 3rd shell has 9 orbitals: 1 from 3s, 3 from 3p, and 5 from 3d.</p> Signup and view all the answers

<p>The greater the charge/mass ratio, the more a particle will deflect; electrons, having a high charge/mass ratio, are deflected the most, while neutrons, having no charge, are undeflected.</p> Signup and view all the answers

<p>[Ar] 3d⁵</p> Signup and view all the answers

<p>A 2s orbital is a 3d sphere that is larger than a 1s orbital.</p> Signup and view all the answers

<p>As electrons are removed, the effective nuclear charge increases, resulting in a stronger attraction between remaining electrons and the nucleus.</p> Signup and view all the answers

<p>Group 14.</p> Signup and view all the answers

<p>The 3px and 3py orbitals are oriented along different axes in three-dimensional space, but both have the same shape.</p> Signup and view all the answers

<p>The first ionization energy is the energy required to remove one mole of electrons from one mole of gaseous atoms to form 1+ charged ions.</p> Signup and view all the answers

<p>The 3s orbital is also a 3d sphere but is larger than both the 1s and 2s orbitals.</p> Signup and view all the answers

<p>Ti²⁺: [Ar] 3d²; Cu⁺: [Ar] 3d¹⁰.</p> Signup and view all the answers

<p>The electronic configuration for Chromium (Cr) is 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d⁵. This deviation occurs because a half-filled d orbital is more stable, prompting one electron from 4s to be transferred to 3d.</p> Signup and view all the answers

<p>The electronic configuration of the sodium ion (Na⁺) is 1s² 2s² 2p⁶, which differs from neutral sodium's configuration of 1s² 2s² 2p⁶ 3s¹ by the loss of one electron from the 3s orbital.</p> Signup and view all the answers

<p>The electronic configuration of Bromide ion (Br⁻) is 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶, while neutral Bromine has 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁵. The Bromide ion has one additional electron in the 4p orbital, achieving a full outer shell.</p> Signup and view all the answers

<p>The electronic configuration of Copper (Cu) is 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d¹⁰. The anomalous configuration occurs because having a completely filled 3d orbital is more stable than following the typical Aufbau principle.</p> Signup and view all the answers

<p>For sodium ions, the electron is removed from the 3s orbital, leading to Na⁺ with configuration 1s² 2s² 2p⁶. In transition metals, electrons are removed first from the 4s orbital before the 3d orbital.</p> Signup and view all the answers

<p>The minimum amount of energy required to remove 1 mole of electrons from 1 mole of gaseous atoms to form 1 mole of 1+ charged gaseous ions.</p> Signup and view all the answers

<p>The electron from element B is removed from a higher energy level compared to A, leading to less energy needed for ionization.</p> Signup and view all the answers

<p>The atomic radius decreases across Period 3 due to increased nuclear charge while shielding remains constant.</p> Signup and view all the answers

<p>Na⁺ (g) → Na²⁺ (g) + e^-</p> Signup and view all the answers

<p>As the atomic radius decreases, more energy is required to remove an electron because the electron is closer to the nucleus.</p> Signup and view all the answers

<p>Aluminum has its outer electron in a higher energy 3p orbital compared to magnesium’s 3s orbital, making it easier to remove.</p> Signup and view all the answers

<p>The shielding effect reduces the effective nuclear charge felt by outer electrons, affecting ionization energy across periods.</p> Signup and view all the answers

<p>First ionization energies increase due to a higher nuclear charge and constant shielding, resulting in a smaller atomic radius.</p> Signup and view all the answers

<p>The primary reason is the increase in nuclear charge across the period, while shielding remains constant.</p> Signup and view all the answers

<p>Shielding increases due to the addition of inner electron shells, making it easier to remove an electron.</p> Signup and view all the answers

<p>Radon (Rn) has the highest first ionization energy.</p> Signup and view all the answers

<p>The equation is: <code>X+(g) → X^2+(g) + e^−</code>.</p> Signup and view all the answers

<p>The removal of an electron is most difficult from F(g).</p> Signup and view all the answers

<p>The possible first element in this sequence is nitrogen (N).</p> Signup and view all the answers

<p>Elements B, J, and R have full outer electron shells.</p> Signup and view all the answers

<p>Atoms of elements D and L contain 2 electrons in their outer shells.</p> Signup and view all the answers

<p>1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹</p> Signup and view all the answers

<p>Chlorine (Cl)</p> Signup and view all the answers

<p>[He] 2s² 2p²</p> Signup and view all the answers

<p>Manganese (Mn)</p> Signup and view all the answers

<p>6 electrons</p> Signup and view all the answers

<p>It indicates that neon has a full outer shell, making it inert.</p> Signup and view all the answers

<p>Nickel (Ni)</p> Signup and view all the answers

<p>Chromium exhibits an electron configuration of 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d⁵, which shows a half-filled d-subshell.</p> Signup and view all the answers

<p>The configuration is 1s² 2s² 2p⁶ 3s², indicating it has 2 valence electrons.</p> Signup and view all the answers

<p>Arsenic (As)</p> Signup and view all the answers