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Questions and Answers
What is the primary basis for organizing elements in the Periodic Table?
What is the primary basis for organizing elements in the Periodic Table?
Which of the following statements about metals is NOT correct?
Which of the following statements about metals is NOT correct?
What is the relative atomic mass of oxygen?
What is the relative atomic mass of oxygen?
What mass unit is one twelfth the mass of a carbon-12 atom called?
What mass unit is one twelfth the mass of a carbon-12 atom called?
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Which property is associated with metalloids?
Which property is associated with metalloids?
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Which scientist is NOT credited with the independent cataloging of elements?
Which scientist is NOT credited with the independent cataloging of elements?
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What reaction characteristic describes how metals behave?
What reaction characteristic describes how metals behave?
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What is the relationship between the mass of a proton and an electron?
What is the relationship between the mass of a proton and an electron?
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What primarily affects the increase in electron affinity across a period?
What primarily affects the increase in electron affinity across a period?
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Which of the following characteristics is NOT associated with non-metals?
Which of the following characteristics is NOT associated with non-metals?
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What type of cation do alkali metals typically form?
What type of cation do alkali metals typically form?
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The most electronegative element is:
The most electronegative element is:
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Which group of metals is characterized by having two electrons in their outer shell?
Which group of metals is characterized by having two electrons in their outer shell?
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What is a common characteristic of transition metals?
What is a common characteristic of transition metals?
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Which statement about halogens is true?
Which statement about halogens is true?
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What happens to the ionic radius when an atom forms a cation?
What happens to the ionic radius when an atom forms a cation?
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What is the effect of increasing nuclear charge on ionization energy across a period?
What is the effect of increasing nuclear charge on ionization energy across a period?
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Which statement about electron affinity is correct?
Which statement about electron affinity is correct?
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How does the atomic radius compare to the cation radius?
How does the atomic radius compare to the cation radius?
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What happens to the first ionization energy as you move down a group in the periodic table?
What happens to the first ionization energy as you move down a group in the periodic table?
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What is the significance of measuring ionization energy experimentally?
What is the significance of measuring ionization energy experimentally?
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Why do anions have a larger ionic radius compared to their atomic radius?
Why do anions have a larger ionic radius compared to their atomic radius?
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What is the characteristic of the second ionization energy compared to the first ionization energy for an atom?
What is the characteristic of the second ionization energy compared to the first ionization energy for an atom?
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How many groups are present in the modern periodic table design?
How many groups are present in the modern periodic table design?
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What is the filling order for the s and p orbitals in the modern periodic table?
What is the filling order for the s and p orbitals in the modern periodic table?
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Which block in the periodic table contains elements with their outermost electrons in the s orbitals?
Which block in the periodic table contains elements with their outermost electrons in the s orbitals?
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What characterizes elements within the same group of the periodic table?
What characterizes elements within the same group of the periodic table?
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What is the total number of columns in the d-block of the periodic table?
What is the total number of columns in the d-block of the periodic table?
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In the context of periodic table organization, what does moving from left to right across a period indicate?
In the context of periodic table organization, what does moving from left to right across a period indicate?
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How many columns are available for f orbitals in the periodic table?
How many columns are available for f orbitals in the periodic table?
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Which group in the periodic table is commonly referred to as group 0?
Which group in the periodic table is commonly referred to as group 0?
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What primarily characterizes the transition metals in the d-block?
What primarily characterizes the transition metals in the d-block?
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How does the atomic radius change as you move down a group in the periodic table?
How does the atomic radius change as you move down a group in the periodic table?
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What effect does the increase in effective nuclear charge have as you move across a period?
What effect does the increase in effective nuclear charge have as you move across a period?
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How do electrons in the same shell affect each other's repulsive forces?
How do electrons in the same shell affect each other's repulsive forces?
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What happens to the ionic radius when an atom gains electrons?
What happens to the ionic radius when an atom gains electrons?
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What is the primary reason for the size increase of an atom as you move down a group?
What is the primary reason for the size increase of an atom as you move down a group?
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Which of the following statements is true regarding the f-block elements?
Which of the following statements is true regarding the f-block elements?
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Why do elements of the d-block show little variation in atomic radii across the series?
Why do elements of the d-block show little variation in atomic radii across the series?
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Study Notes
Medical Chemistry L2
- The lecturer is Professor Dr. Giovanni N. Roviello
- The course is for Geomedi University, Tbilisi, Georgia
- Topic: Periodic Table of Elements
Periodic Table of Elements
- A catalog of all known elements
- Organized by characteristics
- Similar elements in the same column
- Elements with increasing mass placed sequentially
- Developed independently by Dmitri Mendeleev and Lothar Meyer
Arrangement of elements in the periodic table
- Periods: Horizontal rows, increasing atomic size
- Groups: Vertical columns, similar chemical properties (state of matter, reactivity)
Types of Elements
- Metals: Solids at room temperature, good conductors of electricity, malleable, shiny, form positive ions
- Non-metals: Gases or solids at room temperature, poor conductors of electricity, form negative ions
- Metalloids: Have intermediate properties, semiconductors used in technology.
Elementary Properties of atoms-Mass
- The mass of particles are: -Proton: 1.672623 x 10⁻²⁷ kg -Neutron: 1.674929 x 10⁻²⁷ kg -Electron: 9.1093690 x 10⁻³¹ kg
- Proton mass is 1836 times greater than electron mass
Atomic Mass Unit (UMA)
- Atomic masses in kilograms are very small
- Relative atomic masses are compared to a reference value, the atomic mass unit (uma): -One twelfth of the mass of a carbon-12 atom (1.66 x 10⁻²⁷ kg)
- Relates atomic mass to carbon-12
Periodic Table History and Modern Periodic Table
- Mendeleev (1869) based classification on chemical properties
- Meyer (1869) based classification on physical properties
- Modern table reflects atomic structure insights and quantum theory
- Organizes elements according to electron orbital filling principles (Aufbau Principle)
Blocks in the Periodic Table
- Four blocks (s, p, d, f) correspond to orbital types
- Number of columns in each block corresponds to the number of electrons that can be accommodated in the relevant orbital subshells.
- s-block: 2 columns
- p-block: 6 columns
- d-block: 10 columns
- f-block: 14 columns
Groups and Periods in the Periodic Table
- Groups: Columns; Elements share similar outer electron configuration and have similar properties
- Periods: Rows; Atomic number increases from left to right indicating the addition of one proton and electron
Periodic Properties- Atomic Radius
- Half the distance between two identical bonded atoms
- Increases down a group (due to new electron shells)
- Decreases across a period (due to increased nuclear charge, less shielding)
Periodic Properties- Ionic Radius
- Radius of an ion
- Increases down a group; Increases going left
- Decreases going across a period
- Cations (loss of electrons) are smaller; Anions (gain of electrons) are larger
Periodic Properties- Ionization Energy
- Energy required to remove an electron from a neutral atom
- Higher across a period because of stronger attraction to nucleus
- Lower down a group as the atom increases in size and electrons are further from the positively charged nucleus.
Periodic Properties- Electron Affinity
- Energy change associated with acquiring an electron
- Increases across a period (due to increased nuclear charge)
- Decreases down a group as the atom size increases, decreased attraction
Electronegativity
- Atom's ability to attract electrons in a bond
- Based on values of first ionization energy and electron affinity
- Highest electronegativity is for fluorine
- Lowest is for cesium
Classification of Elements
- Metals (e.g., Iron, Copper, Gold)
- Non-metals (e.g., Oxygen, Chlorine)
- Metalloids (e.g., Silicon, Boron)
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Description
Explore the intricate organization of the Periodic Table of Elements in this Medical Chemistry L2 quiz. Understand the classification of elements by their properties, including metals, non-metals, and metalloids, as well as the concepts of periods and groups. This quiz will enhance your knowledge of the fundamental building blocks of matter.