Types of Bonds
What type of bond occurs when electrons are transferred from one atom to another?
A: Ionic bond
Name this compound:CoCl3
A:Cobalt (III) Chloride
What model shows all the energy levels and electrons of an atom?
A: Bohr model
What is the trend for atomic radius as you move across a period?
A: It decreases
What does Coulomb’s Law describe?
A: The attraction between charged particles
What type of bond involves sharing of electrons between nonmetals?
A: Covalent bond
Write the formula for calcium and oxygen.
A: CaO
What model uses dots to represent valence electrons in bonds?
A: Lewis dot structure
What is the trend for ionization energy as you move down a group?
A: It decreases
According to Coulomb’s Law, how does distance affect attraction?
A: Greater distance → weaker attraction
What type of bond forms a “sea of electrons” allowing conductivity and malleability?
A: Metallic bond
What is the name of P4O5?
A: Tetraphosphorous Pentaoxide
What is the molecular shape of CO₂? Why?
A: Linear
Define electronegativity.
A: The ability of an atom to attract electrons in a bond
Why does MgO have a higher melting point than NaCl?
A: Mg²⁺ and O²⁻ have higher charges, creating stronger attractions
Compare the melting points of ionic and covalent compounds — which tends to be higher and why?
A: Ionic compounds; stronger electrostatic forces hold ions tightly together
Write the formula for dinitrogen tetraoxide.
A: N₂O₄
What is the molecular shape of H₂O, and why?
A: Bent; caused by lone pairs pushing bonding pairs
Is a cation smaller than its neutral atom? Y/N, Why?
A: Yes. It loses electrons, reducing the number of electrons needed to hold onto.
What two factors affect the strength of attraction according to Coulomb’s Law?
A: Charge and distance
List one key property for each: metallic, ionic, and covalent compounds.
A: Metallic – conducts electricity; Ionic – high melting point; Covalent – low melting point
Write the formula for Copper (II) Chlorite
A: Cu(ClO2)2
What is the repeating, 3D pattern formed by ions in an ionic solid called?
A: Crystal lattice
Which element is the most electronegative, greatest ionization energy, and largest atomic radii, on the periodic table?
A: Fluorine, Helium, Francium.
Explain how Coulomb’s Law relates to lattice energy.
A: Lattice energy measures ionic bond strength; stronger charges and smaller ions increase lattice energy