Fundamentals of Medicinal and Pharmaceutical Chemistry

Podcast

Play an AI-generated podcast conversation about this lesson

Questions and Answers

Which statement best describes John Dalton's view of a chemical reaction?

Reactions can lead to the transformation of one element into another.

Atoms combine in a fixed ratio to form compounds but do not rearrange.

Atoms are created and destroyed during chemical reactions.

Chemical reactions involve the rearrangement of atoms without their creation or destruction. (correct)

What was J.J. Thomson's significant contribution to atomic theory?

Determination of the electron's charge-to-mass ratio using cathode ray tubes. (correct)

Discovery of the neutron and its properties.

Identification of the atom as the smallest indivisible unit.

Introduction of the concept of the electron cloud model.

How did Rutherford's model of the atom differ from Thomson's plum-pudding model?

Rutherford proposed that electrons are dispersed throughout the nucleus.

Rutherford claimed that positive and negative charges are equally dense throughout the atom.

Rutherford suggested a dense nucleus where positive charges are concentrated. (correct)

Rutherford dismissed the existence of protons within atoms entirely.

Why is the plum-pudding model significant in the development of atomic theory?

It represented a major shift in thinking, highlighting the existence of subatomic particles. Signup and view all the answers

Which of the following concepts did Bohr contribute to atomic theory?

The idea that electrons occupy fixed orbits around the nucleus. Signup and view all the answers

What is the charge of a cation?

Positive charge Signup and view all the answers

How is Na+ formed from a neutral sodium atom?

By losing one electron Signup and view all the answers

Which ion is most prevalent as a negatively charged ion (anion) in blood?

Cl- Signup and view all the answers

What happens to the number of protons and electrons in an atom when it becomes a cation?

Number of protons remains the same, electrons decrease Signup and view all the answers

What is the electronic configuration of Na+?

1s2 2s2 2p6 Signup and view all the answers

Which of the following ions must have gained electrons to become negatively charged?

Cl- Signup and view all the answers

What is the result when an atom gains one electron?

It becomes an anion Signup and view all the answers

For the ion K+, how does the electron count compare to a neutral potassium atom?

Fewer electrons than protons Signup and view all the answers

What role does the nucleus play when an atom becomes an ion?

The nucleus remains unaffected Signup and view all the answers

Which is NOT a principle relevant to atomic structure?

Law of Conservation of Mass Signup and view all the answers

Which principle states that an increase in precision in measuring the position of a particle results in less precision in measuring its momentum?

Uncertainty Principle Signup and view all the answers

What does the Schrodinger Wave Equation describe regarding electrons in an atom?

The probability of finding an electron within a specific position Signup and view all the answers

Which statement best describes an atomic orbital?

A region in space with high probability of finding an electron Signup and view all the answers

How do atomic orbitals vary?

In size, energy, shape, and orientation Signup and view all the answers

During which conference was the wave-particle duality of electrons highlighted?

Solvay Conference 1927 Signup and view all the answers

What is NOT a characteristic of atomic orbitals?

Restricted to spherical shapes Signup and view all the answers

Which orbital represents the highest electron density probability in a three-dimensional atom?

s orbital Signup and view all the answers

What does the Heisenberg Uncertainty Principle imply for measuring particles?

Simultaneous measurements of momentum and position have limits of accuracy Signup and view all the answers

Which of the following is true about electronic configurations in atomic orbitals?

Some orbitals can accommodate multiple electrons Signup and view all the answers

What was one of the significant outcomes of the Solvay Conference 1927?

Debating the dual nature of light and matter Signup and view all the answers

Which of the following best describes the Pauli Exclusion Principle?

No two electrons in the same atom can have the same set of quantum numbers. Signup and view all the answers

What characterizes the shapes of s, p, and d orbitals?

s orbitals are spherical, p orbitals are dumbbell-shaped, and d orbitals have complex shapes. Signup and view all the answers

Which statement correctly describes Dalton's Atomic Theory?

Compounds are formed by a specific arrangement of atoms in definite ratios. Signup and view all the answers

What is the electronic configuration of a neutral oxygen atom?

1s² 2s² 2p⁴ Signup and view all the answers

Which principle explains why electrons fill the lowest energy orbitals first?

Aufbau Principle Signup and view all the answers

In a chemical context, what defines a cation?

An atom that has more protons than electrons. Signup and view all the answers

What does Hund's Rule of Maximum Multiplicity state?

Electrons will occupy degenerate orbitals singly before any pairing occurs. Signup and view all the answers

Which scientist is associated with the development of wave-particle duality?

Louis de Broglie Signup and view all the answers

What is the name of the first subatomic particle discovered?

Electron Signup and view all the answers

Who proposed the plum pudding model of the atom?

J.J. Thomson Signup and view all the answers

What is credited with the discovery of the atom's nucleus?

Rutherford's gold foil experiment Signup and view all the answers

What is the positively charged particle found in the nucleus?

Proton Signup and view all the answers

Who proposed that electrons move in circular orbits around the nucleus and these orbits have specific energies?

Niels Bohr Signup and view all the answers

What did Einstein demonstrate regarding light?

Light can have both wave and particle properties Signup and view all the answers

What is the concept that suggests matter and light can exhibit both wave and particle properties?

Wave-particle duality Signup and view all the answers

Who put forward the uncertainty principle?

Werner Heisenberg Signup and view all the answers

What did Schrodinger develop to describe the probability of finding an electron within a specific position in an atom?

Mathematical functions Signup and view all the answers

What does 'spd(f)' notation represent in atomic orbitals?

Energy and size of the orbital Signup and view all the answers

What does the superscript in electronic configurations represent?

The number of electrons in the orbital Signup and view all the answers

Name the three rules used to determine the electronic configuration of elements?

Pauli Exclusion Principle, Aufbau Principle, and Hund's Rule Signup and view all the answers

According to the Pauli Exclusion Principle, how many electrons can occupy an orbital?

2 Signup and view all the answers

Which rule states that electrons will fill the lowest available energy levels first?

Aufbau Principle Signup and view all the answers

What does Hund's Rule dictate regarding electron filling in orbitals of equal energy?

Electrons fill orbitals singly before pairing up Signup and view all the answers

Which of the following statements correctly describes the relationship between the principal quantum number and the energy level of an orbital?

Higher the principal quantum number, higher the energy level Signup and view all the answers

What is the term used for the outermost electron in an atom?

Valence electron Signup and view all the answers

An ion is an atom or group of atoms that has a neutral charge

False Signup and view all the answers

What is the term for an ion with a net positive charge?

Cation Signup and view all the answers

What type of ion is formed when an atom gains electrons?

Anion Signup and view all the answers

What is the main positive ion found in blood?

Sodium ion (Na+) Signup and view all the answers

What is considered the main cation in cell fluid?

Potassium ion (K+) Signup and view all the answers

What is the name of the dense central core within an atom?

Nucleus Signup and view all the answers

Which of the following scientists is credited with the discovery of the photoelectric effect?

Einstein Signup and view all the answers

According to the Uncertainty Principle, what cannot be known simultaneously with certainty?

The position and momentum of a particle Signup and view all the answers

What is the name of the equation that describes the probability of finding an electron within a particular position in an atom?

Schrödinger Wave Equation Signup and view all the answers

The Pauli Exclusion Principle states that no more than two electrons can occupy the same orbital, and those electrons must have opposite spins.

True Signup and view all the answers

What is the name of the principle that describes the filling of atomic orbitals in order of increasing energy?

Aufbau Principle Signup and view all the answers

What is the name of the rule that states that electrons will fill orbitals of equal energy individually before pairing up?

Hund's Rule Signup and view all the answers

What is the name of the outermost electron in an atom that is involved in chemical bonding?

Valence electron Signup and view all the answers

What is the electronic configuration of the sodium ion (Na+)?

1s2 2s2 2p6 Signup and view all the answers

What is the electronic configuration of potassium ion (K+)?

1s2 2s2 2p6 3s2 3p6 Signup and view all the answers

What is the electronic configuration of chlorine ion (Cl-)?

1s2 2s2 2p6 3s2 3p6 Signup and view all the answers

Which type of elements are most commonly found in the human body?

Transition metals Signup and view all the answers

The electronic configuration of chromium (Cr) is an exception to the Aufbau Principle because its 3d orbitals are half-filled.

True Signup and view all the answers

The electronic configuration of copper (Cu) is an exception to the Aufbau Principle because its 3d orbitals are completely filled.

True Signup and view all the answers

Formation of ions only involves changes in the number of electrons in an atom, not the number of protons.

True Signup and view all the answers

What primarily causes the decrease in ionization energy as you move down a group in the periodic table?

Increased shielding from inner-shell electrons Signup and view all the answers

Which group of elements is known to have the lowest ionization energy?

Alkali metals Signup and view all the answers

What is the concept of electron affinity primarily related to?

The energy change when an atom in the gaseous state accepts an electron Signup and view all the answers

Which statement correctly compares the electronegativity of elements?

Electronegativity increases from left to right across a period Signup and view all the answers

Which of the following trends is seen in ionization energies across the periodic table?

Ionization energy decreases from right to left in a period Signup and view all the answers

What is the primary reason fluorine has the highest electronegativity?

It has a high nuclear charge and little shielding. Signup and view all the answers

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

It decreases due to increased atomic radius. Signup and view all the answers

Which element has the highest ionization energy in the following list?

Fluorine Signup and view all the answers

Which statement best defines electron affinity?

The energy change when an atom gains electrons. Signup and view all the answers

Comparing the electronegativities of F, O, N, and C, what trend is observed?

F > O > N > C Signup and view all the answers

What happens to the ionic radius of an element when it forms a cation?

It decreases due to increased nuclear charge. Signup and view all the answers

Which ion has a smaller ionic radius: Na+ or Mg2+?

Mg2+ because it has a higher nuclear charge. Signup and view all the answers

What is the significance of the ionic radius trend in relation to nuclear charge?

An increased nuclear charge causes a decrease in ionic radius. Signup and view all the answers

Why do isoelectronic ions like Na+ and Mg2+ have different ionic radii?

The ion with the higher nuclear charge has a smaller radius. Signup and view all the answers

Which statement best describes the formation of a unipositive ion?

The loss of an electron decreases the size of the ion. Signup and view all the answers

Among the following ions, which has the largest ionic radius?

Cl- Signup and view all the answers

How does the ionic radius of a dipositive ion compare to a unipositive ion?

It is smaller due to greater nuclear charge. Signup and view all the answers

When comparing ionic radii across a group in the periodic table, what trend is typically observed?

Ionic radii increase from top to bottom. Signup and view all the answers

What happens to ionization energy as the distance between the nucleus and the outermost electron increases?

It decreases Signup and view all the answers

Which elements generally have the highest ionization energy?

Noble gases Signup and view all the answers

What does a positive electron affinity value indicate?

Energy is required to add an electron Signup and view all the answers

How is electron affinity defined in relation to energy changes?

The negative of the energy change when an electron is accepted Signup and view all the answers

What is the relationship between electronegativity and bond electron sharing?

Electronegativity impacts how equally electrons are shared in a bond Signup and view all the answers

What does electronegativity primarily measure?

The ability of an atom to attract electrons in a chemical bond Signup and view all the answers

Why is fluorine considered the most electronegative element?

It has a high nuclear charge with minimal shielding Signup and view all the answers

What relationship exists between electronegativity, electron affinity, and ionization energy?

Electronegativity is related to both electron affinity and ionization energy Signup and view all the answers

Which of the following trends in electronegativity is observed across a period on the periodic table?

Electronegativity increases as you move from left to right Signup and view all the answers

What is indicated by the dipole in the bond between hydrogen and fluorine?

Fluorine pulls electrons toward itself, creating a slight charge difference Signup and view all the answers

What is the significance of groups in the periodic table?

Elements in the same group show similar chemical properties. Signup and view all the answers

Which statement correctly describes the conduction properties of metals and nonmetals?

Metals are good conductors of heat and electricity, while nonmetals are not. Signup and view all the answers

What does the effective nuclear charge (Zeff) account for?

The attractive force between the nucleus and valence electrons after considering shielding. Signup and view all the answers

Why are valence electrons essential in chemical reactions?

They are involved in the bonding and exchange interactions between atoms. Signup and view all the answers

What defines the shielding effect in an atom?

The blocking of nuclear charge by inner-shell electrons from outer-shell electrons. Signup and view all the answers

What generally happens to the reactivity of Group I and Group VII elements?

They are the most reactive elements in their respective groups. Signup and view all the answers

How does the distance of electrons from the nucleus affect the attraction between them?

Greater distance decreases the attraction between electrons and the nucleus. Signup and view all the answers

What can be inferred about the nature of chemical reactions based on valence electrons?

Chemical reactions primarily involve changes in the arrangement of valence electrons. Signup and view all the answers

What property distinguishes metals from non-metals and metalloids in the periodic table?

Electrical conductivity Signup and view all the answers

Which of the following best defines ‘effective nuclear charge’?

The net positive charge experienced by an electron in a multi-electron atom Signup and view all the answers

What happens to the effective nuclear charge (Zeff) as you move across a period from left to right?

Zeff increases because of a greater number of protons. Signup and view all the answers

How does ionization energy typically change when moving across a period in the periodic table?

It increases Signup and view all the answers

Which group in the periodic table contains highly reactive elements typically found in nature only as compounds?

Halogens Signup and view all the answers

How does the atomic radius change as you move down a group in the periodic table?

The atomic radius increases because electrons are added to higher energy levels. Signup and view all the answers

What is the primary distinction between lanthanides and actinides in the periodic table?

Their electron configurations Signup and view all the answers

What effect do valence electrons have on the effective nuclear charge (Zeff) experienced by other valence electrons?

Valence electrons do not shield each other effectively. Signup and view all the answers

According to Slater's rules, what do these rules primarily account for?

The effective shielding of electrons in different orbitals. Signup and view all the answers

Which of the following statements is true about the atomic radius of elements in the periodic table?

It decreases across a period Signup and view all the answers

What is the atomic radius defined as?

Half the distance between the centers of two adjacent nuclei. Signup and view all the answers

What arrangement method did Mendeleev use for his periodic table?

Increasing atomic mass Signup and view all the answers

Which of the following elements is considered an alkali metal?

Sodium Signup and view all the answers

What happens to the ionic radius when an atom forms an anion?

The ionic radius increases due to added electrons and electron-electron repulsion. Signup and view all the answers

How does the effective nuclear charge (Zeff) change as you move down a group in the periodic table according to Slater's rules?

Zeff decreases due to increased shielding by inner shell electrons. Signup and view all the answers

What direct effect does increasing atomic number (Z) have on atomic radius as you move across a period?

Atomic radius decreases due to increasing effective nuclear charge. Signup and view all the answers

How does the radius of a dinegative ion compare to that of a uninegative ion?

It is larger than the radius of a uninegative ion. Signup and view all the answers

What effect does increasing the nuclear charge have on ionization energy across a period?

Ionization energy increases due to greater attraction between electrons and the nucleus. Signup and view all the answers

Which statement is true regarding the first ionization energy (IE1)?

It is the energy needed to remove the first electron from a gaseous atom. Signup and view all the answers

What happens to ionization energy as you go down a group in the periodic table?

It decreases as electrons enter a higher energy level. Signup and view all the answers

Why does F- have a smaller size compared to O2-?

F- has a larger nuclear charge compared to O2-. Signup and view all the answers

What is the trend in first ionization energy (IE1) when moving across a period?

IE1 increases because of greater effective nuclear charge. Signup and view all the answers

What distinguishes the second ionization energy (IE2) from the first ionization energy (IE1)?

IE2 occurs after the atom has already lost one electron. Signup and view all the answers

Which statement about isoelectronic species is correct?

Isoelectronic species have the same number of electrons. Signup and view all the answers

Study Notes