Atomic Structure
This positively charged subatomic particle is found inside the nucleus and determines an element's identity.
Proton.
The reaction type where a solid product is formed from a solution.
precipitation reaction.
A liquid with a pH value of 3 is classified as this
acid
Classify this substance: Liquid pure water, which consists of two different types of elements chemically bonded together.
Compound
___ N2 + ___ H2 → 2 NH3
1,3
Atoms of the same element that have the same number of protons but different numbers of neutrons.
Isotopes
The state symbol denoted by (aq) in a chemical equation means the substance is dissolved in this.
water
The two main products formed when an acid reacts completely with a base in a neutralization reaction.
salt and water
Classify this particle: A single, neutral sodium particle containing 11 protons and 11 electrons.
atom
Balance this classic neutralization equation:
HCl + NaOH → NaCl + H2O
Balanced!
An atom that has gained or lost electrons, giving it an overall positive or negative charge.
Ion
Ions in a reaction that remain unchanged in solution on both sides of the equation and do not participate in the actual chemical change.
spectator ions
The color that universal indicator or litmus paper turns in a strongly alkaline/basic solution (pH 12–14).
blue
Assign the charge: A neutral calcium atom (Ca) loses 2 electrons during a chemical reaction to achieve a stable full outer shell. What is its resulting charge?
+2
Write the complete ionic equation for the following molecular reaction by splitting all aqueous compounds into their separate ions:
NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq)
Na+(aq) + Cl-(aq) + Ag+(aq) + NO3-(aq) → AgCl(s) + Na+(aq) + NO3-(aq)
Electrons located in the outermost shell of an atom that are involved in chemical bonding.
Valence electrons.
The coefficients needed to balance this equation:
__Fe+__O2 -> __ Fe2O3
4,3,2
An acid is defined as a molecule or ion that acts as a donor of these particles.
H+ ion
Classify this species: Sulfate (SO42-), which consists of multiple sulfur and oxygen atoms bonded together with an overall negative charge.
polyatomic ion
Identify the two spectator ions in this ionic equation:
K+(aq) + I-(aq) + Pb2+(aq) + NO3-(aq) → PbI2(s) + K+(aq) + NO3-(aq)
K+ (Potassium) and NO3- (Nitrate)
The trend on the periodic table where an atom's ability to attract shared electrons increases as you move across a period to the right and up a group.
Electronegativity.
In a single displacement reaction, a free metal can only displace another metal from a compound if it sits higher on this list.
Reactivity series
On the pH scale (which ranges from 0 to 14), a solution that is completely neutral—such as pure drinking water—has this exact pH value.
7
Assign the correct classification (Atom, Element Molecule, Compound, or Ion) to each of these 4 chemical symbols in order:
Fe
O2
Cl-
Atom / Element
Element Molecule
Compound
Ion (or Anion)
Write the final net ionic equation for the precipitation reaction between aqueous Silver Nitrate and aqueous Sodium Chloride, which forms solid Silver Chloride.
Ag+(aq) + Cl-(aq) → AgCl(s)