Chemistry: Atomic and Ionic Radius Concepts
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Questions and Answers

What makes metallic compounds strong?

  • The low melting points and malleability of metals
  • The sea of electrons that hold the atoms together (correct)
  • The arrangement of atoms in a cubic structure
  • The presence of ionic bonds between metal atoms

How do the size of metal atoms affect the strength of metallic bonds?

  • Larger atoms create stronger bonds due to increased size
  • Size does not affect the strength of metallic bonds
  • Smaller atoms can pack together more tightly, leading to stronger bonds (correct)
  • Only the shape of the atom influences bond strength

Which of the following properties is not characteristic of metals?

  • Low thermal conductivity (correct)
  • High melting points
  • High electrical conductivity
  • Malleable and ductile

What role do valence electrons play in metallic bonding?

<p>More valence electrons typically lead to stronger metallic bonds (C)</p> Signup and view all the answers

Which bond forms first in a double bond?

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

Why are metals considered ductile and malleable?

<p>The lattice structure allows atoms to slide past each other (D)</p> Signup and view all the answers

What is the primary reason for metals having high melting points?

<p>The strength of metallic bonds between atoms (C)</p> Signup and view all the answers

What is the relationship between bond strength and bond length?

<p>Stronger bonds have shorter bond lengths. (D)</p> Signup and view all the answers

What distinguishes a pi bond from a sigma bond?

<p>A sigma bond forms first, and a pi bond is weaker due to different orbital overlaps (D)</p> Signup and view all the answers

Which of the following correctly describes a characteristic of weaker bonds?

<p>Weaker bonds have longer bond lengths. (A)</p> Signup and view all the answers

What prefix is used to indicate one atom of the first element in a binary molecular compound?

<p>None (D)</p> Signup and view all the answers

What is the correct naming convention for the acid formed from hydrochloric acid?

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

Which polyatomic ion, when forming an oxyacid, results in an acid that ends with -ous?

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

Which of the following is an example of a molecule that forms with an incomplete octet?

<p>BF₂ (D)</p> Signup and view all the answers

In which scenario can an element's octet be expanded beyond eight electrons?

<p>Elements in Period 3 and beyond. (D)</p> Signup and view all the answers

What does a free radical represent in molecular terms?

<p>A molecule with an odd number of electrons. (B)</p> Signup and view all the answers

What property of ionic compounds is primarily due to the strong bonds between ions?

<p>High melting and boiling points (D)</p> Signup and view all the answers

Which statement correctly describes how ionic compounds conduct electricity?

<p>They conduct electricity when melted or dissolved in water. (B)</p> Signup and view all the answers

When writing the formula for binary ionic compounds, what must be ensured?

<p>The overall charge of the compound must be neutral. (C)</p> Signup and view all the answers

What is the correct nomenclature for the compound FeCl₃?

<p>Iron(III) Chloride (B)</p> Signup and view all the answers

Which polyatomic ion example is correctly paired with its formula?

<p>Ammonium - NH₄⁺ (C)</p> Signup and view all the answers

In the construction of polyatomic compounds, what is the primary concern regarding charges?

<p>The charges must be balanced to be zero. (A)</p> Signup and view all the answers

Which of the following describes the structure of metallic compounds?

<p>Organized lattice allowing slide past each other (D)</p> Signup and view all the answers

Which property of metals is a direct result of their unique bonding and structure?

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

Flashcards

Metallic Bond Strength

The strength of the bond between metal atoms in a metallic compound, determined by the number of valence electrons and the size of the metal atoms.

Metallic Lattice Structure

A regular, repeating pattern of metal atoms arranged in a lattice, which allows for flexibility and ductility in metals.

Sea of Electrons

A cloud of delocalized valence electrons that are free to move within the lattice structure of a metal, forming strong, flexible bonds.

Metallic Properties (Conductivity)

Metals have high electrical and thermal conductivity because the delocalized electrons can easily move, transporting heat and electricity.

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Metallic Properties (Ductility/Malleability)

Atoms in a metal can slide past each other without breaking the bonds, which makes metals ductile (stretchy) and malleable (bendable).

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Covalent Bond (Sigma)

The strongest type of covalent bond, formed when two atomic orbitals overlap head-on.

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Covalent Bond (Pi)

A weaker covalent bond formed when two p orbitals overlap side-by-side, appearing in double or triple covalent bonds.

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Covalent Bond (Strength/Length/Energy)

The strength of a covalent bond is related to its length and dissociation energy: stronger bonds have shorter lengths and higher dissociation energies.

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Ionic Compound Properties

Ionic compounds are hard, brittle, have high melting and boiling points, and conduct electricity when melted or dissolved in water.

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Metallic Bond

A bond formed when metal atoms share their valence electrons in a 'sea' of electrons.

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Metallic Structure

Metal atoms arranged in a regular, organized lattice that allows atoms to slide past each other.

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Metallic Properties

Metals are conductive, malleable, ductile, strong, and shiny due to their bonding and structure.

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Binary Compound Formula

A compound of two elements, balancing charges to make it neutral.

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Polyatomic Ion

A charged group of atoms.

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Oxidation State

The charge an atom would have if all the bonds were ionic.

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Balancing Charges (Ionic Compounds)

Ensuring the total positive charge equals the total negative charge in an ionic compound.

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Bond Length and Dissociation Energy

Stronger bonds have shorter lengths and higher dissociation energies, while weaker bonds have longer lengths and lower dissociation energies.

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Binary Molecular Compound Naming

Naming binary (two-element) molecules involves using prefixes to indicate the number of atoms of each element (e.g., 'di' for two, 'tri' for three, etc.). The first element is named as-is, and the second element's name ends in '-ide'.

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Binary Acid Naming

Naming acids with two elements (hydrogen and a nonmetal) uses the prefix 'hydro-' followed by the nonmetal name that ends in '-ic', and the word ‘acid'.

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Oxyacid Naming

Naming oxyacids (acids with hydrogen, oxygen, and a nonmetal or polyatomic ion), look to the suffix of the polyatomic ion. If the polyatomic ion ends in -ate, the acid ends in -ic; if the polyatomic ion ends in –ite, the acid ends in -ous. Add the word “acid.”

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Incomplete Octet

Some elements like boron and beryllium can form stable molecules with fewer than 8 valence electrons.

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Expanded Octet

Elements from Period 3 and beyond can have more than 8 electrons in their valence shell because of available d orbitals.

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Odd Number of Electrons

Some molecules, like NO2, have an odd number of electrons, making it impossible to satisfy the octet rule for all atoms.

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Octet Rule Exceptions

Elements like boron and period 3 and beyond can form stable compounds that don't follow the octet rule of having exactly 8 electrons in their valence shell.

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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!

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