Chemistry Exam 2
Studied by 0 people
Call with Kai
Knowt Play
Learn
Practice Test
Spaced Repetition
Match
Flashcards1/33
There's no tags or description
Looks like no tags are added yet.
Name | Mastery | Learn | Test | Matching | Spaced |
|---|
No study sessions yet.
34 Terms
Q: What is the formula for maximum electrons per energy level?
A: Max electrons=2n2
Q: What is a valence electron?
A: An electron in the outermost shell of an atom.
Q: What happens when an atom gains electrons?
A: It becomes a negatively charged anion.
Q: What happens when an atom loses electrons?
A: It becomes a positively charged cation.
Q: How do you calculate ionic charge?
A: Ionic charge = Number of protons − Number of electrons
Q: How is an ionic bond formed?
A: Through the transfer of electrons between a metal and a nonmetal.
Q: How is a covalent bond formed?
A: Through the sharing of electrons between nonmetals.
Q: What are key traits of ionic compounds?
A: High melting point, conducts electricity when dissolved.
Q: What are key traits of covalent compounds?
A: Lower melting point, does not conduct electricity.
Q: How do you name a binary ionic compound?
A: Metal name + nonmetal root + “-ide” (e.g., NaCl = sodium chloride)
Q: How do you name a compound with a transition metal?
A: Use Roman numerals to indicate the metal’s charge (e.g., FeCl₂ = Iron(II) chloride)
Q: How do you name a compound with a polyatomic ion?
A: Keep the polyatomic ion name intact (e.g., NaNO₃ = sodium nitrate)
Q: What is a polyatomic ion?
A group of atoms bonded together with an overall charge.
Q: Give examples of polyatomic ions.
A: NO₃⁻ (nitrate), SO₄²⁻ (sulfate), NH₄⁺ (ammonium)
Q: What are the steps to draw a Lewis structure?
A: Count valence electrons, choose central atom, pair electrons to form bonds, redraw as lines.
Q: What is the octet rule?
A: Atoms tend to gain, lose, or share electrons to achieve 8 in their valence shell.
Q: What determines molecular geometry?
A: The number of bonding and nonbonding electron groups around the central atom.
Q: What is the geometry and bond angle for 4 electron groups, all bonding?
A: Tetrahedral, 109.5°
Q: What is the geometry for 4 electron groups with 1 lone pair?
A: Trigonal pyramidal
Q: What is the geometry for 4 electron groups with 2 lone pairs?
A: Bent
Q: What is electronegativity?
A: An atom’s ability to attract electrons in a bond.
Q: What is the bond type if electronegativity difference is < 0.5?
A: Nonpolar covalent
Q: What is the bond type if electronegativity difference is between 0.5 and 2.0?
A: Polar covalent
Q: What is the bond type if electronegativity difference is > 2.0?
A: Ionic
Q: What makes a molecule polar?
A: Lone pairs on the central atom or different outer atoms.
Q: What is the weakest IMF?
A: London dispersion forces
Q: What is the strongest dipole-dipole force?
A: Hydrogen bonding (H bonded to F, O, or N)
Q: What is the strongest overall IMF?
A: Ionic attraction (between full charges)
Q: What are alkanes?
A: Saturated hydrocarbons with only single bonds.
Q: Name the first 5 straight-chain alkanes.
A: Methane (CH₄), Ethane (C₂H₆), Propane (C₃H₈), Butane (C₄H₁₀), Pentane (C₅H₁₂)
Q: What does a line structure represent?
A: Each bend or end is a carbon atom; hydrogens are implied.
Q: What is a constitutional isomer?
A: Molecules with the same formula but different connectivity.
Q: What is a cycloalkane?
A: A ring-shaped saturated hydrocarbon.
Q: Give examples of cycloalkanes.
A: Cyclopropane (C₃H₆), Cyclobutane (C₄H₈), Cyclopentane (C₅H₁₀)
Note 
Flashcards (22)