Fundamentals of Medicinal and Pharmaceutical Chemistry

<p>It represented a major shift in thinking, highlighting the existence of subatomic particles. (D)</p> Signup and view all the answers

<p>The idea that electrons occupy fixed orbits around the nucleus. (D)</p> Signup and view all the answers

<p>Positive charge (B)</p> Signup and view all the answers

<p>By losing one electron (B)</p> Signup and view all the answers

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

<p>Number of protons remains the same, electrons decrease (B)</p> Signup and view all the answers

<p>1s2 2s2 2p6 (B)</p> Signup and view all the answers

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

<p>It becomes an anion (D)</p> Signup and view all the answers

<p>Fewer electrons than protons (C)</p> Signup and view all the answers

<p>The nucleus remains unaffected (D)</p> Signup and view all the answers

<p>Law of Conservation of Mass (C)</p> Signup and view all the answers

<p>Uncertainty Principle (D)</p> Signup and view all the answers

<p>The probability of finding an electron within a specific position (C)</p> Signup and view all the answers

<p>A region in space with high probability of finding an electron (C)</p> Signup and view all the answers

<p>In size, energy, shape, and orientation (D)</p> Signup and view all the answers

<p>Solvay Conference 1927 (D)</p> Signup and view all the answers

<p>Restricted to spherical shapes (D)</p> Signup and view all the answers

<p>s orbital (C)</p> Signup and view all the answers

<p>Simultaneous measurements of momentum and position have limits of accuracy (B)</p> Signup and view all the answers

<p>Some orbitals can accommodate multiple electrons (D)</p> Signup and view all the answers

<p>Debating the dual nature of light and matter (C)</p> Signup and view all the answers

<p>No two electrons in the same atom can have the same set of quantum numbers. (C)</p> Signup and view all the answers

<p>s orbitals are spherical, p orbitals are dumbbell-shaped, and d orbitals have complex shapes. (C)</p> Signup and view all the answers

<p>Compounds are formed by a specific arrangement of atoms in definite ratios. (C)</p> Signup and view all the answers

<p>1s² 2s² 2p⁴ (B)</p> Signup and view all the answers

<p>Aufbau Principle (D)</p> Signup and view all the answers

<p>An atom that has more protons than electrons. (A)</p> Signup and view all the answers

<p>Electrons will occupy degenerate orbitals singly before any pairing occurs. (C)</p> Signup and view all the answers

<p>Louis de Broglie (B)</p> Signup and view all the answers

<p>Electron</p> Signup and view all the answers

<p>J.J. Thomson</p> Signup and view all the answers

<p>Rutherford's gold foil experiment</p> Signup and view all the answers

<p>Proton</p> Signup and view all the answers

<p>Niels Bohr</p> Signup and view all the answers

<p>Light can have both wave and particle properties</p> Signup and view all the answers

<p>Wave-particle duality</p> Signup and view all the answers

<p>Werner Heisenberg</p> Signup and view all the answers

<p>Mathematical functions</p> Signup and view all the answers

<p>Energy and size of the orbital</p> Signup and view all the answers

<p>The number of electrons in the orbital</p> Signup and view all the answers

<p>Pauli Exclusion Principle, Aufbau Principle, and Hund's Rule</p> Signup and view all the answers

<p>2 (B)</p> Signup and view all the answers

<p>Aufbau Principle</p> Signup and view all the answers

<p>Electrons fill orbitals singly before pairing up (D)</p> Signup and view all the answers

<p>Higher the principal quantum number, higher the energy level (C)</p> Signup and view all the answers

<p>Valence electron</p> Signup and view all the answers

<p>False (B)</p> Signup and view all the answers

<p>Cation (B)</p> Signup and view all the answers

<p>Anion (A)</p> Signup and view all the answers

<p>Sodium ion (Na+)</p> Signup and view all the answers

<p>Potassium ion (K+)</p> Signup and view all the answers

<p>Nucleus</p> Signup and view all the answers

<p>Einstein (B)</p> Signup and view all the answers

<p>The position and momentum of a particle (D)</p> Signup and view all the answers

<p>Schrödinger Wave Equation</p> Signup and view all the answers

<p>True (A)</p> Signup and view all the answers

<p>Aufbau Principle</p> Signup and view all the answers

<p>Hund's Rule</p> Signup and view all the answers

<p>Valence electron</p> Signup and view all the answers

<p>1s2 2s2 2p6 (B)</p> Signup and view all the answers

<p>1s2 2s2 2p6 3s2 3p6 (B)</p> Signup and view all the answers

<p>1s2 2s2 2p6 3s2 3p6 (B)</p> Signup and view all the answers

<p>Transition metals</p> Signup and view all the answers

<p>True (A)</p> Signup and view all the answers

<p>True (A)</p> Signup and view all the answers

<p>True (A)</p> Signup and view all the answers

<p>Increased shielding from inner-shell electrons (B), Increased distance between the nucleus and outermost electrons (C)</p> Signup and view all the answers

<p>Alkali metals (C)</p> Signup and view all the answers

<p>The energy change when an atom in the gaseous state accepts an electron (B)</p> Signup and view all the answers

<p>Electronegativity increases from left to right across a period (A), Electronegativity decreases down a group (B)</p> Signup and view all the answers

<p>Ionization energy decreases from right to left in a period (A), Ionization energy tends to increase from left to right across a period (B)</p> Signup and view all the answers

<p>It has a high nuclear charge and little shielding. (A)</p> Signup and view all the answers

<p>It decreases due to increased atomic radius. (A)</p> Signup and view all the answers

<p>Fluorine (D)</p> Signup and view all the answers

<p>The energy change when an atom gains electrons. (A)</p> Signup and view all the answers

<p>F &gt; O &gt; N &gt; C (C)</p> Signup and view all the answers

<p>It decreases due to increased nuclear charge. (D)</p> Signup and view all the answers

<p>Mg2+ because it has a higher nuclear charge. (C)</p> Signup and view all the answers

<p>An increased nuclear charge causes a decrease in ionic radius. (B)</p> Signup and view all the answers

<p>The ion with the higher nuclear charge has a smaller radius. (A)</p> Signup and view all the answers

<p>The loss of an electron decreases the size of the ion. (D)</p> Signup and view all the answers

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

<p>It is smaller due to greater nuclear charge. (C)</p> Signup and view all the answers

<p>Ionic radii increase from top to bottom. (A)</p> Signup and view all the answers

<p>It decreases (B)</p> Signup and view all the answers

<p>Noble gases (D)</p> Signup and view all the answers

<p>Energy is required to add an electron (A)</p> Signup and view all the answers

<p>The negative of the energy change when an electron is accepted (C)</p> Signup and view all the answers

<p>Electronegativity impacts how equally electrons are shared in a bond (A)</p> Signup and view all the answers

<p>The ability of an atom to attract electrons in a chemical bond (D)</p> Signup and view all the answers

<p>It has a high nuclear charge with minimal shielding (C)</p> Signup and view all the answers

<p>Electronegativity is related to both electron affinity and ionization energy (D)</p> Signup and view all the answers

<p>Electronegativity increases as you move from left to right (D)</p> Signup and view all the answers

<p>Fluorine pulls electrons toward itself, creating a slight charge difference (B)</p> Signup and view all the answers

<p>Elements in the same group show similar chemical properties. (D)</p> Signup and view all the answers

<p>Metals are good conductors of heat and electricity, while nonmetals are not. (C)</p> Signup and view all the answers

<p>The attractive force between the nucleus and valence electrons after considering shielding. (B)</p> Signup and view all the answers

<p>They are involved in the bonding and exchange interactions between atoms. (B)</p> Signup and view all the answers

<p>The blocking of nuclear charge by inner-shell electrons from outer-shell electrons. (C)</p> Signup and view all the answers

<p>They are the most reactive elements in their respective groups. (B)</p> Signup and view all the answers

<p>Greater distance decreases the attraction between electrons and the nucleus. (B)</p> Signup and view all the answers

<p>Chemical reactions primarily involve changes in the arrangement of valence electrons. (D)</p> Signup and view all the answers

<p>Electrical conductivity (B)</p> Signup and view all the answers

<p>The net positive charge experienced by an electron in a multi-electron atom (C)</p> Signup and view all the answers

<p>Zeff increases because of a greater number of protons. (B)</p> Signup and view all the answers

<p>It increases (A)</p> Signup and view all the answers

<p>Halogens (B)</p> Signup and view all the answers

<p>The atomic radius increases because electrons are added to higher energy levels. (B)</p> Signup and view all the answers

<p>Their electron configurations (C)</p> Signup and view all the answers

<p>Valence electrons do not shield each other effectively. (C)</p> Signup and view all the answers

<p>The effective shielding of electrons in different orbitals. (B)</p> Signup and view all the answers

<p>It decreases across a period (B)</p> Signup and view all the answers

<p>Half the distance between the centers of two adjacent nuclei. (C)</p> Signup and view all the answers

<p>Increasing atomic mass (C)</p> Signup and view all the answers

<p>Sodium (C)</p> Signup and view all the answers

<p>The ionic radius increases due to added electrons and electron-electron repulsion. (A)</p> Signup and view all the answers

<p>Zeff decreases due to increased shielding by inner shell electrons. (D)</p> Signup and view all the answers

<p>Atomic radius decreases due to increasing effective nuclear charge. (B)</p> Signup and view all the answers

<p>It is larger than the radius of a uninegative ion. (D)</p> Signup and view all the answers

<p>Ionization energy increases due to greater attraction between electrons and the nucleus. (D)</p> Signup and view all the answers

<p>It is the energy needed to remove the first electron from a gaseous atom. (B)</p> Signup and view all the answers

<p>It decreases as electrons enter a higher energy level. (D)</p> Signup and view all the answers

<p>F- has a larger nuclear charge compared to O2-. (C)</p> Signup and view all the answers

<p>IE1 increases because of greater effective nuclear charge. (D)</p> Signup and view all the answers

<p>IE2 occurs after the atom has already lost one electron. (B)</p> Signup and view all the answers

<p>Isoelectronic species have the same number of electrons. (D)</p> Signup and view all the answers

Scientists like Thompson, Rutherford, Bohr, Einstein, deBroglie, Heisenberg, and Schrodinger contributed to our understanding of atomic structure.

Regions of space where electrons are likely to be found around the atomic nucleus.

Different shapes and energies of electron orbitals.

No two electrons in an atom can have the same set of four quantum numbers.

Electrons fill the lowest energy levels first.

Electrons occupy empty orbitals before pairing up in the same orbital.

Arrangement of electrons in atomic orbitals.

Describing electron distribution for the first 30 Periodic Table elements and their ions.

A process that involves the separation, combination, or rearrangement of atoms. Atoms are not created or destroyed.

J.J. Thomson discovered and identified the first subatomic particle, the electron, through experiments using cathode ray tubes.

Thomson proposed that electrons are embedded within a uniform, positively charged sphere, similar to plums in a pudding.

Rutherford discovered the atom's dense, positively charged nucleus through his famous gold foil experiment. He proposed that the nucleus contains positively charged protons.

Bohr's model focuses on how electrons are arranged outside the nucleus of an atom.

A cation forms when a neutral atom loses one or more electrons, resulting in a net positive charge.

An anion forms when a neutral atom gains one or more electrons, resulting in a net negative charge.

A sodium atom (Na) loses one electron to become a sodium cation (Na+).

A chlorine atom (Cl) gains one electron to become a chloride anion (Cl-).

A potassium atom (K) loses one electron to form a potassium cation (K+).

Electrons and other small particles can behave like both waves and particles.

It's impossible to know both the position and momentum of a particle precisely at the same time.

A mathematical equation that describes the probability of finding an electron in a specific location within an atom.

An important meeting of physicists that discussed new ideas in quantum physics.

A type of atomic orbital with a spherical shape around the nucleus.

A measure of how quickly and in what direction an electron is moving.

A measure of the quantity of motion of an object.

A group of atomic orbitals within an atom, all of which have the same energy.

Electrons are arranged in atomic orbitals, which are regions of space around the nucleus where an electron is likely to be found.

There are s orbitals (spherical), p orbitals (dumbbell shaped), and d orbitals (more complex shapes).

Each orbital can hold a maximum of two electrons, according to the Pauli Exclusion Principle.

Electrons fill orbitals in increasing energy order, starting with the lowest energy levels (Aufbau principle).

Electrons fill orbitals individually before pairing up within the same orbital. This maximizes spin multiplicity, leading to stability.

A set of principles that describe the fundamental nature of atoms, proposing that elements are made of tiny, indivisible particles called atoms, and atoms of the same element are identical. Compounds form when atoms of different elements combine in specific ratios.

Thomson discovered the electron, the first subatomic particle, using cathode ray tubes. He determined the ratio of electric charge to mass for an electron.

Thomson envisioned the atom as a positively charged sphere with negatively charged electrons embedded within it, like plums in a pudding.

Rutherford fired alpha particles (positively charged) at a thin gold foil and observed that some particles were deflected, suggesting the presence of a dense, positively charged nucleus within the atom.

Rutherford proposed that the atom has a small, dense, positively charged nucleus at its center, where protons reside, and electrons orbit around it.

Bohr proposed that electrons orbit the nucleus in specific energy levels, or orbits, with each orbit having a distinct energy.

Einstein explained that light, while behaving like a wave, can also act as particles called photons, which can knock electrons out of a material.

de Broglie suggested that matter, like light, can exhibit wave-like properties, meaning that particles, like electrons, can behave as waves.

There are different types of atomic orbitals: s orbitals are spherical, p orbitals are dumbbell shaped, and d orbitals have more complex shapes. Each type has a different energy level.

Transition metals are elements that have partially filled d orbitals. They have unique properties due to the filling of these d orbitals.

Elements like chromium (Cr) and copper (Cu) don't always follow the typical filling rules for orbitals. This is because half-filled or completely filled d orbitals provide extra stability.

Valence electrons are the electrons in the outermost energy level of an atom. These electrons are involved in chemical bonding.

The minimum energy required to remove an electron from a gaseous atom in its ground electronic state.

Ionization energy is influenced by factors like the distance between the nucleus and the outermost electron, the number of protons in the nucleus, and the shielding effect of inner electrons.

The change in energy when an electron is added to a neutral atom in its gaseous state to form a negative ion.

A measure of an atom's ability to attract shared electrons in a chemical bond.

Electronegativity increases across a period and decreases down a group in the periodic table.

Fluorine has a high nuclear charge, small atomic radius, and little shielding. It readily gains electrons due to its high electron affinity and high ionization energy.

Electronegativity increases across a period from left to right. This is because the number of protons in the nucleus increases, leading to a stronger attraction for electrons.

Electronegativity decreases down a group. This is because the atomic radius increases, and the outer electrons are farther from the nucleus, leading to weaker attraction.

A dipole forms when there's an uneven distribution of electron density in a molecule due to differences in electronegativity.

The distance from the nucleus to the outermost electron in an ion.

Ionic radius increases as you move down a group in the periodic table and decreases as you move across a period.

Ions with the same number of electrons.

A greater nuclear charge pulls electrons closer to the nucleus, resulting in a smaller ionic radius.

A dipositive ion (e.g., Mg²⁺) is smaller than a unipositive ion (e.g., Na⁺) with the same number of electron shells.

When comparing ions, the ion with the smaller nuclear charge and more electron shells will be larger.

The Periodic Table organizes all known elements based on their properties and atomic structure, making it easier to predict and understand their behavior.

Periods are horizontal rows and represent the number of electron shells, while groups are vertical columns and indicate elements with similar chemical properties.

Metals are generally shiny, malleable, and good conductors of heat and electricity, non-metals are dull, brittle, and poor conductors, while metalloids have properties of both.

The net positive charge experienced by an electron in an atom. It's a measure of how strongly the nucleus pulls on an electron.

The Modern Periodic Table arranges elements by increasing atomic number, with elements in the same group (column) having similar chemical properties due to their similar valence electron configurations.

Valence electrons are the outermost electrons in an atom that participate in chemical reactions by sharing or exchanging with other atoms.

A higher Zeff means a stronger attraction between the nucleus and the valence electrons, leading to a smaller atomic radius and increased ionization energy.

Metals are good conductors of heat and electricity due to their free-flowing valence electrons. Non-metals typically conduct poorly because their valence electrons are tightly held.

A group (column) on the periodic table consists of elements with similar chemical properties because they have the same number of valence electrons.

A period (row) in the periodic table represents elements with the same number of electron shells, resulting in trends in atomic size and other properties.

Elements in Group I (alkali metals) and Group VII (halogens) are the most reactive because they easily gain or lose electrons to achieve a stable electron configuration.

Zeff increases across a period because the number of protons in the nucleus increases, making the attraction stronger.

Zeff remains roughly constant down a group because the increase in shielding from added electrons cancels out the increase from more protons.

Atomic radius decreases across a period due to the increase in Zeff, pulling electrons closer to the nucleus.

Atomic radius increases down a group because electrons are added to higher energy levels farther from the nucleus.

Anions are larger than their neutral atoms because of the added electrons, while cations are smaller because of the electron loss.

The ionic radius increases as you move down a group in the periodic table.

The ionic radius decreases as you move across a period in the periodic table.

The minimum energy required to remove an electron from a gaseous atom in its ground state.

Ionization energy increases as you move across a period in the periodic table.

Ionization energy decreases as you move down a group in the periodic table.

Fluorine has the highest electronegativity due to its small size, high nuclear charge, and strong attraction for electrons.

Electronegativity increases as you move from left to right across a period in the periodic table.

Electronegativity decreases as you move down a group in the periodic table.