Electron Configuration and Electromagnetic Radiation

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Questions and Answers

Which electron configuration represents the valence shell of the transition metal iron (Fe)?

4s 3d (correct)

3s 3p

4s 4p

3s 3d

What is the correct electron configuration for Ti3+, when starting from the neutral titanium atom?

1s2 2s2 2p6 3s2 3p6 4s1 3d2

1s2 2s2 2p6 3s2 3p6 3d1 (correct)

1s2 2s2 2p6 3s2 3p6

1s2 2s2 2p6 3s2 3p6 4s2 3d3

In which of the following cases is the electron configuration of the ion isoelectronic with that of noble gas?

8O2- (correct)

11Na

17Cl+

19K+

Which statement about the removal of electrons from transition metals is true?

Electrons in the ns orbital are removed before any (n-1)d electrons. Signup and view all the answers

What is the total number of valence electrons in nickel (Ni)?

10 Signup and view all the answers

What is the relationship between wavelength and frequency in electromagnetic radiation?

Wavelength increases as frequency decreases. Signup and view all the answers

What is the value of Planck's constant?

6.62 x 10^-34 Js Signup and view all the answers

In the Bohr model of the hydrogen atom, what does the ground state refer to?

The lowest possible energy level an electron can be at. Signup and view all the answers

Which equation represents the relationship between energy and frequency?

E = hf Signup and view all the answers

What type of spectrum does hydrogen emit?

Line spectrum Signup and view all the answers

How is energy defined in terms of allowable energy levels for an electron in a hydrogen atom?

Energy levels are quantized and fixed to specific values. Signup and view all the answers

What is the formula for calculating the frequency of radiation when given the wavelength?

n = c/l Signup and view all the answers

Which quantity is NOT a property of electromagnetic radiation?

Charge Signup and view all the answers

What is the formula for calculating the radius of an electron's orbit?

rn = 0.5 x n² Å Signup and view all the answers

When an electron transitions from a higher energy level to a lower one, what happens to the energy?

Energy is emitted Signup and view all the answers

What is the energy difference (DE) when an electron transitions from n=4 to n=2?

-4.1 x 10-19 J Signup and view all the answers

Using the de Broglie hypothesis, which statement is true about particle behavior?

Particles can exhibit wave behavior Signup and view all the answers

What is the wavelength of light emitted when an electron transitions from n=4 to n=2?

4.86 x 10-7 m Signup and view all the answers

In the context of the hydrogen line spectrum, which value represents the final energy level in visible transitions?

nf = 2 Signup and view all the answers

What happens to the electron's energy when it absorbs a photon during a transition?

Energy increases Signup and view all the answers

What constants are used in calculating the wavelength of emitted light?

h and C Signup and view all the answers

What values can the orbital quantum number ℓ take when the principal quantum number n=4?

0,1,2,3,4 Signup and view all the answers

Which is the correct name of the sub-level for quantum numbers n=3 and ℓ=2?

3d Signup and view all the answers

When the orbital quantum number ℓ = 1, what values can the magnetic quantum number mℓ take?

-1,0,1 Signup and view all the answers

Which of the following statements is true about the magnetic quantum number (mℓ)?

It can take values of -ℓ to +ℓ. Signup and view all the answers

According to the Aufbau principle, what determines the order in which electrons fill orbitals?

Energy levels, increasing n + ℓ. Signup and view all the answers

What does Hund's Rule state about the distribution of electrons in degenerate orbitals?

Electrons fill each orbital one by one and then pair up. Signup and view all the answers

What principle explains why no two electrons can have the same set of quantum numbers in an atom?

Pauli's Exclusion Principle Signup and view all the answers

In the context of electronic configurations, which orbital has a higher energy level than 3p?

4s Signup and view all the answers

What is the formula for calculating the effective nuclear charge (Zeff)?

Zeff = Z - S Signup and view all the answers

As you move from left to right across a period in the periodic table, what happens to Zeff?

Zeff increases Signup and view all the answers

How does Zeff change when moving down a group in the periodic table?

Zeff remains constant Signup and view all the answers

Calculate Zeff for the sodium ion 11Na+.

9 Signup and view all the answers

What does the atomic size (or radius) refer to?

The half distance of closest approach between two identical atoms Signup and view all the answers

Which of the following elements has the highest effective nuclear charge based on the information provided?

17Cl Signup and view all the answers

If an atom has an atomic number of 13 and 10 inner electrons, what is its effective nuclear charge?

3 Signup and view all the answers

In a multi-electron atom, which statement is true about Zeff?

It is the net positive charge felt by the outermost electrons Signup and view all the answers

What happens to atomic size when moving from left to right along a period in the periodic table?

Atomic size decreases due to increased core charge. Signup and view all the answers

Which of the following correctly describes ionization energy as you move down a group in the periodic table?

Ionization energy decreases due to increasing atomic size and weaker attraction. Signup and view all the answers

Why are cations smaller than the atoms from which they are formed?

The excess of protons draws the outer electrons closer to the nucleus. Signup and view all the answers

What trend occurs in electronegativity as you move across a period from left to right?

Electronegativity increases due to increased core charge. Signup and view all the answers

Which statement accurately describes ionization energy as atomic size increases?

Ionization energy decreases because electrons are easier to detach. Signup and view all the answers

When evaluating the size of anions compared to the parent atoms, what can be said?

Anions are larger due to increased repulsion between electrons. Signup and view all the answers

What is the primary reason for the increase in ionization energy as you go from left to right in a period?

Decreased atomic size increases the attraction of electrons to the nucleus. Signup and view all the answers

Which of the following affects electronegativity the least?

Number of valence electrons. Signup and view all the answers

Study Notes

Introduction to Quantum Theory and Atomic Properties

Atomic orbitals are regions in space with a high probability of finding an electron.
Quantum numbers (n, l, ml) describe atomic orbitals and their electrons.
Principal quantum number (n) indicates the main energy level.
Orbital quantum number (l) describes the shape of the orbital sublevels.
Magnetic quantum number (ml) indicates the orientation of orbitals in space.
Electron spin quantum number (ms) defines the direction of electron spin.

Electromagnetic Radiation (Light)

Wavelength (λ) is the distance between crests of a wave.
Frequency (ν) is the number of complete cycles per second.
Speed of light (c) is constant (3 × 10⁸ m/s).
The relationship between these properties: ν = c/λ

The Continuous and Line Spectrum of Light

A continuous spectrum displays a range of wavelengths without distinct lines.
A line spectrum shows discrete lines of specific wavelengths.
Hydrogen's spectrum is a line spectrum, indicating quantized energy level transitions.

The Wave-Particle Duality of Light

Planck's constant (h) is associated with quantized energy changes in atoms.
Energy is quantized, meaning atoms can only absorb or emit specific amounts of energy.
Light consists of photons, which have both wave-like and particle-like properties.
The energy of a photon is = hv = hc/λ where (h) is Planck's constant

Bohr Model of the Hydrogen Atom

Hydrogen atoms have quantized energy levels for electron orbits.
The ground state is the lowest energy level (n=1) for the electron.
Excited states are higher energy levels (n>1) where electrons are not in the ground state.
The energy levels depend on a constant (RE) and principal quantum number (n).

Transition Between Energy Levels

Electrons move between energy levels by absorbing or emitting photons.
The energy of the photon equals the difference in energy between the energy levels.
Emission of light happens when electrons move to a lower energy level.
Absorption of light occurs when electrons move to a higher energy level.

Electron Configurations

Aufbau Principle: Electrons fill orbitals in order of increasing energy.
Hund's Rule: In orbitals of equal energy, electrons first fill singly with parallel spins and fill in pairs only when necessary.
Pauli Exclusion Principle: No two electrons in an atom can have the same set of four quantum numbers.
Transition elements or metals: Electrons fill (n-1)d before the ns orbital.

Effective Nuclear Charge (Z_eff)

Effective nuclear charge is the net positive charge felt by an electron in a multi-electron atom.
It's calculated by subtracting the number of inner electrons (core electrons—S) from the atomic number.
Effective nuclear charge increases across a period, resulting in smaller atomic sizes.

Atomic Radius

Atomic size is the half the distance between the nuclei of two bonded identical atoms.
Atomic radius decreases across a period and increases down a group of the periodic table.

Ionization Energy

Ionization energy is the energy required to remove an electron from a gaseous atom.
Ionization energy increases across a period and decreases down a group.

Electronegativity

Electronegativity is the tendency of an atom to attract electrons towards it in a chemical bond.
Electronegativity increases across a period and decreases down a group.

Electronic Configuration of Ions

Electrons are first removed from the highest energy orbitals (except transition metals) when forming cations.
Electrons are added to the lowest energy orbitals when forming anions.
Ions often have the same electronic configuration (isoelectronic) to another atom or ion.

Electronic Configuration of Transition Metals and Ions

Electrons in the ns orbital are removed before any electrons in the (n-1)d orbitals when forming ions.

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Description

This quiz covers key concepts related to electron configurations, particularly for transition metals like iron and titanium. It also addresses important principles of electromagnetic radiation, including the relationship between frequency and wavelength, as well as the Bohr model of the hydrogen atom. Test your understanding of these fundamental topics in chemistry and physics.