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Questions and Answers
What makes metallic compounds strong?
What makes metallic compounds strong?
How do the size of metal atoms affect the strength of metallic bonds?
How do the size of metal atoms affect the strength of metallic bonds?
Which of the following properties is not characteristic of metals?
Which of the following properties is not characteristic of metals?
What role do valence electrons play in metallic bonding?
What role do valence electrons play in metallic bonding?
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Which bond forms first in a double bond?
Which bond forms first in a double bond?
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Why are metals considered ductile and malleable?
Why are metals considered ductile and malleable?
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What is the primary reason for metals having high melting points?
What is the primary reason for metals having high melting points?
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What is the relationship between bond strength and bond length?
What is the relationship between bond strength and bond length?
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What distinguishes a pi bond from a sigma bond?
What distinguishes a pi bond from a sigma bond?
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Which of the following correctly describes a characteristic of weaker bonds?
Which of the following correctly describes a characteristic of weaker bonds?
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What prefix is used to indicate one atom of the first element in a binary molecular compound?
What prefix is used to indicate one atom of the first element in a binary molecular compound?
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What is the correct naming convention for the acid formed from hydrochloric acid?
What is the correct naming convention for the acid formed from hydrochloric acid?
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Which polyatomic ion, when forming an oxyacid, results in an acid that ends with -ous?
Which polyatomic ion, when forming an oxyacid, results in an acid that ends with -ous?
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Which of the following is an example of a molecule that forms with an incomplete octet?
Which of the following is an example of a molecule that forms with an incomplete octet?
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In which scenario can an element's octet be expanded beyond eight electrons?
In which scenario can an element's octet be expanded beyond eight electrons?
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What does a free radical represent in molecular terms?
What does a free radical represent in molecular terms?
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What property of ionic compounds is primarily due to the strong bonds between ions?
What property of ionic compounds is primarily due to the strong bonds between ions?
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Which statement correctly describes how ionic compounds conduct electricity?
Which statement correctly describes how ionic compounds conduct electricity?
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When writing the formula for binary ionic compounds, what must be ensured?
When writing the formula for binary ionic compounds, what must be ensured?
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What is the correct nomenclature for the compound FeCl₃?
What is the correct nomenclature for the compound FeCl₃?
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Which polyatomic ion example is correctly paired with its formula?
Which polyatomic ion example is correctly paired with its formula?
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In the construction of polyatomic compounds, what is the primary concern regarding charges?
In the construction of polyatomic compounds, what is the primary concern regarding charges?
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Which of the following describes the structure of metallic compounds?
Which of the following describes the structure of metallic compounds?
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Which property of metals is a direct result of their unique bonding and structure?
Which property of metals is a direct result of their unique bonding and structure?
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Study Notes
Atomic Radius
- Decreases across a period (→): More protons pull electrons closer to the nucleus.
- Increases down a group (↓): More electron shells are added, increasing size.
Ionic Radius
- Cations (positive ions): Smaller than their parent atoms. Losing electrons reduces electron-electron repulsion.
- Anions (negative ions): Larger than their parent atoms. Gaining electrons increases repulsion, expanding the ion.
- Decreases across a period (→) for ions of the same charge: Higher nuclear charge pulls electrons closer.
- Increases down a group (↓): More electron shells increase size.
Ionization Energy (IE)
- Increases across a period (→): Electrons are held more tightly due to higher nuclear charge.
- Decreases down a group (↓): Electrons are farther from the nucleus and easier to remove.
Electronegativity
- Increases across a period (→) Atoms want to complete their octet (non-metals attract electrons strongly).
- Decreases down a group (↓): Larger atoms have weaker attraction for bonding electrons.
Quantum Numbers
- The energy level or shell of an electron. How far the electron is from the nucleus
- Each energy level (n) can hold 2n² electrons.
- Energy level (n): Subshells: Number of orbitals: Max electrons.
- n=1: s: 1: 2
- n=2: s,p: 1+3=4: 8
- n=3: s,p,d: 1+3+5=9: 18
- n=4: s,p,d,f: 1+3+5+7=16: 32
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Description
Test your understanding of atomic and ionic radius, ionization energy, and electronegativity with this quiz. Explore how these properties change across periods and down groups in the periodic table. Perfect for chemistry students looking to reinforce their knowledge!
