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Questions and Answers
Which elements if organized by mass would be in reverse order?
Which elements if organized by mass would be in reverse order?
Who is primarily credited with the development of the periodic table?
Who is primarily credited with the development of the periodic table?
Which scientist used X-ray spectroscopy to determine atomic numbers?
Which scientist used X-ray spectroscopy to determine atomic numbers?
What is a scientific law best known for?
What is a scientific law best known for?
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What is a scientific theory based upon?
What is a scientific theory based upon?
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Which of the following is NOT a predicted element by Mendeleev?
Which of the following is NOT a predicted element by Mendeleev?
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What are the valence electrons for main-group elements?
What are the valence electrons for main-group elements?
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Which of these elements did Moseley predict by observing gaps in atomic number sequence?
Which of these elements did Moseley predict by observing gaps in atomic number sequence?
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What is the van der Waals radius of an atom defined as?
What is the van der Waals radius of an atom defined as?
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Which of the following species is larger in size?
Which of the following species is larger in size?
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Which of the following isoelectronic species would have the smallest radius?
Which of the following isoelectronic species would have the smallest radius?
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How is a covalent radius determined?
How is a covalent radius determined?
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When an electron is removed from an atom, forming a cation, is the ionization energy positive or negative?
When an electron is removed from an atom, forming a cation, is the ionization energy positive or negative?
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Why is it necessary to average several measurements of different compounds to determine a reliable atomic radius?
Why is it necessary to average several measurements of different compounds to determine a reliable atomic radius?
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Which of the following generally decreases as you move down a group in the periodic table?
Which of the following generally decreases as you move down a group in the periodic table?
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What happens to the atomic radius as you move down a group in the periodic table?
What happens to the atomic radius as you move down a group in the periodic table?
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Which of the following generally increases as you move from left to right across a period in the periodic table?
Which of the following generally increases as you move from left to right across a period in the periodic table?
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What happens to the atomic radius as you move to the right across a period in the periodic table?
What happens to the atomic radius as you move to the right across a period in the periodic table?
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Considering the exceptions to first ionization energy trends, which element has a lower first ionization energy than expected?
Considering the exceptions to first ionization energy trends, which element has a lower first ionization energy than expected?
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What primary factor largely determines atomic radius?
What primary factor largely determines atomic radius?
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Which of the following statements is true regarding successive ionization energies?
Which of the following statements is true regarding successive ionization energies?
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Which of the following is a key determining factor for the increase in atomic radius moving down a group?
Which of the following is a key determining factor for the increase in atomic radius moving down a group?
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What does the term 'effective nuclear charge' refer to?
What does the term 'effective nuclear charge' refer to?
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How does the radius of a Cl atom compare to a Cl$-$ ion?
How does the radius of a Cl atom compare to a Cl$-$ ion?
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Why is the electron in a helium ion ($He^+$) more strongly attracted to the nucleus than the electron in a hydrogen atom (H)?
Why is the electron in a helium ion ($He^+$) more strongly attracted to the nucleus than the electron in a hydrogen atom (H)?
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What is the effect of core electrons on the outermost electrons in an atom?
What is the effect of core electrons on the outermost electrons in an atom?
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Which statement best describes the behavior of outermost electrons regarding nuclear charge?
Which statement best describes the behavior of outermost electrons regarding nuclear charge?
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Based on the periodic trends, how does the atomic radius change as you move down a group/column in the periodic table?
Based on the periodic trends, how does the atomic radius change as you move down a group/column in the periodic table?
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Based on periodic trends, how does atomic radius change as you move across a period (from left to right) in the periodic table?
Based on periodic trends, how does atomic radius change as you move across a period (from left to right) in the periodic table?
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Which option correctly describes how the radius of a cation compares to its corresponding neutral atom?
Which option correctly describes how the radius of a cation compares to its corresponding neutral atom?
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Which of the following pairs of elements would have the smallest difference in atomic radii?
Which of the following pairs of elements would have the smallest difference in atomic radii?
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Which element has the largest atomic radius?
Which element has the largest atomic radius?
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Based on periodic trends, which element has the higher first ionization energy, aluminum (Al) or sulfur (S)?
Based on periodic trends, which element has the higher first ionization energy, aluminum (Al) or sulfur (S)?
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Based on periodic trends, which element has the higher first ionization energy, arsenic (As) or antimony (Sb)?
Based on periodic trends, which element has the higher first ionization energy, arsenic (As) or antimony (Sb)?
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Based on periodic trends, which element has the higher first ionization energy, nitrogen (N) or silicon (Si)?
Based on periodic trends, which element has the higher first ionization energy, nitrogen (N) or silicon (Si)?
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Based on periodic trends, which element has the higher first ionization energy, oxygen (O) or chlorine (Cl)?
Based on periodic trends, which element has the higher first ionization energy, oxygen (O) or chlorine (Cl)?
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What is the definition of electron affinity?
What is the definition of electron affinity?
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According to the provided text, which of the following is generally true about electron affinity?
According to the provided text, which of the following is generally true about electron affinity?
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Which of the following statements is true regarding the metallic character of elements?
Which of the following statements is true regarding the metallic character of elements?
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In the context provided, what does a positive electron affinity value suggest?
In the context provided, what does a positive electron affinity value suggest?
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Which of the following represents the general formula for the reaction between a metal and a halogen?
Which of the following represents the general formula for the reaction between a metal and a halogen?
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In the reaction $2 Fe(s) + 3 Cl_2(g) \longrightarrow 2 FeCl_3(s)$, what is reduced?
In the reaction $2 Fe(s) + 3 Cl_2(g) \longrightarrow 2 FeCl_3(s)$, what is reduced?
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What is the product when a halogen reacts with hydrogen?
What is the product when a halogen reacts with hydrogen?
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What type of compounds are formed when different halogens are reacted together?
What type of compounds are formed when different halogens are reacted together?
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Which of the following noble gases has the highest first ionization energy?
Which of the following noble gases has the highest first ionization energy?
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Which of the noble gases has the largest atomic radius?
Which of the noble gases has the largest atomic radius?
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Which noble gas has a density closest to 1 g/L at STP?
Which noble gas has a density closest to 1 g/L at STP?
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Which noble gas has the lowest boiling point?
Which noble gas has the lowest boiling point?
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Study Notes
Chapter 8 Outline
- This outline details the structure and properties of the elements along with examples and trends
- Topics include nerve signal transmission, development of the periodic table, electron configurations, and periodic trends in atomic size and effective nuclear charge.
8.1 Nerve Signal Transmission
- Nerve signals are transmitted throughout the body, mediated by ion transport across cell membranes
- Tiny pumps are found in cell membranes
- These pumps transport ions like sodium (Na+) and potassium (K+) across ion channels which are in membranes and these ions are pumped in opposite directions
- Sodium ions pumped out of cells; potassium ions are pumped into cells
- This creates a chemical gradient where the sodium concentration is higher outside the cell than inside the cell. The opposite is true for potassium.
8.2 The Development of the Periodic Table
- The periodic table was developed primarily by Dmitri Mendeleev, with similar work from Julius Lothar Meyer.
- Mendeleev's table arranged elements by increasing atomic mass
- Elements with similar properties grouped together in the same columns.
- Mendeleev's table allowed predictions about the existence and characteristics of yet undiscovered elements. These were known as gallium and germanium.
8.3 Electron Configurations, Valence Electrons, and the Periodic Table
- Valence electrons are located in the outermost principal energy levels.
- For transition elements, outermost d electrons are also considered valence electrons.
8.4 The Explanatory Power of the Quantum-Mechanical Model
- Model explains why certain elements exhibit similar chemical properties
- Electron configurations of atoms are key in predicting how elements react with each other and their properties
- Model explains the periodic repeating patterns of chemical properties across the periodic table.
8.5 Periodic Trends in the Size of Atoms and Effective Nuclear Charge
- Atomic size trends (i.e., Atomic radii) : size of atoms or atomic radius increases going down a group (column) in the periodic table; and decreases going across a period(row) from left to right in the table.
- van der Waals radius: one-half the distance between adjacent nuclei in a solid.
- Covalent radius: one- half the distance between the nuclei of two single atoms joined together.
- Trend of atomic radius explained by the filling of electron orbitals and the attraction between the electrons and the nucleus.
- Effective nuclear charge (Zeff): inward pull of the nucleus on the outermost electrons, taking into account that electrons in the inner energy levels shield electrons further out from the positive pull of the nucleus.
8.6 Ionic Radii
- Cations are smaller than their corresponding atoms
- Anions are larger than their corresponding atoms
8.7 Ionization Energy
- Ionization energy: energy needed to remove an electron from an atom or ion in its gaseous state
- First ionization energy: energy required to remove the first electron
- Removing an electron requires energy.
- This trend is affected by effective nuclear charge, atomic size and electron shielding.
8.8 Electron Affinities and Metallic Character
- Electron affinity: energy released when an electron is added to a neutral atom in its gaseous state
- Metallic character: ability of an atom to lose electrons
- Trend is affected by effective nuclear charge, atomic size and electron shielding.
8.9 Some Examples of Periodic Chemical Behavior: The Alkali Metals, the Halogens, and the Noble Gases
- Alkali Metals (Group 1): highly reactive, readily lose one electron to form a positive cation
- Halogens (Group 17): highly reactive, readily gain one electron to form an anion
- Noble Gases (Group 18): very unreactive, have a completely filled outer electron shell.
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Description
Test your knowledge on the periodic table and the principles of atomic structure with this quiz. Explore questions related to atomic mass, discoverers, and electron configurations. Perfect for chemistry students looking to reinforce their understanding of the subject.
