Pre-AP Chemistry Exam Review

Practice vocabulary flashcards generated from lecture notes and practice exam questions covering atomic structure, the periodic table, chemical bonding, gas laws, and thermodynamics.

Group 14 Metalloid

Silicon

Valence Electrons Commonality

Elements in the same group have the same number of valence electrons.

Negative Ion Formation

An element that gains an electron to form an ion.

I-131 and I-133 Classification

Isotopes of the same element

Proton

A particle with a charge that is equal in magnitude but opposite in sign compared to an electron.

Carbon-14 Protons

6 protons

Carbon-14 Neutrons

8 neutrons

Carbon-14 Electrons

6 electrons

Carbon-13 Neutrons

7 neutrons

Calcium (Ca) Atomic Symbol

An element that has 20 neutrons and a mass number of 40.

Atomic Nucleus Charge

The nucleus contains all the positive charge of an atom.

Atomic Volume

The majority of an atom's volume is accounted for by electrons surrounding the nucleus.

Earliest Atomic Model

Hard-sphere model

Intermediate Atomic Model (History)

Electron-shell model

Most Recent Atomic Model

Wave-mechanical model

Modern Atom Model

Electrons are likely to be found in orbitals around the nucleus.

Electrically Neutral Atom

The number of protons equals the number of electrons.

Uranium Constant

All atoms of uranium have the same atomic number.

Fewest Protons Sample

$^{232}Th$ (Thorium)

Potassium Excited State Configuration

2-8-7-2

Manganese (Mn) Identity

An element with 30 neutrons and a mass number of 55.

Carbon Octet Requirement

Carbon needs 4 more electrons to give it a complete octet.

Fluorine Ground State Configuration

2-7

Group 17 Diatomic Gases

The group in the Periodic Table containing elements that are all diatomic gases.

Group 17 Name

Halogens

Group 2 Ion Charge

$$2+$$

Group 16 commonality

They all have 6 valence electrons.

Group 18 Reactivity

The least reactive elements on the Periodic Table.

Boron Location

Group 13, Period 2

Rhenium (Re) Property

The element with the highest melting point according to Table S.

Fluorine Chemical Similarity

Reacts in a manner most similar to Chlorine.

Modern Periodic Table Arrangement

Elements are arranged in order of increasing atomic number.

Magnesium Ion Radius

Smaller than the radius of a neutral Magnesium atom.

Metalloids List

Boron (B), Silicon (Si), Germanium (Ge), and Arsenic (As).

Krypton Classification

Noble gas

Bromine (Br) Ionization Energy

Requires the greatest amount of energy to remove the most loosely bound electron among Br, Sr, K, and Sb.

Lowest Electronegativity (N, C, O, F)

Carbon

NaOH Gram-Formula Mass

$$40\,g$$

$Na_2CO_3 \cdot 10H_2O$ Gram-Formula Mass

$$286\,g$$

Physical Change Example

$H_2O(s)$ melts to $H_2O(l)$

Greatest Entropy Phase

Gas phase

DE Segment (Cooling Curve)

Represents a time when both the liquid and solid phases were present.

Standard Heat Release Calculation (Transcript Value)

$481\,joules$ is released by $10.00\,g$ of water dropping from $20.0^{\circ}C$ to $10.0^{\circ}C$.

293K to Celsius Conversion

$$20^{\circ}C$$

Magnesium and Oxygen Reaction Type

Composition or Synthesis (Transcript check: single replacement was marked in Q47 distractors but MgO formation is composition).

Phase with Greatest Kinetic Energy

Gas phase

Boiling (Segment D)

The phase change occurring at $100^{\circ}C$ for water.

Heat to Boil 10.0g Water

$$22.6\,kJ$$

Endothermic Reaction Description

Absorbs heat energy

Phosphorus and Oxygen Bond Type

Covalent bond

HCl Molecular Property

Symmetrical and nonpolar (per transcript answer for Q58).

Iron Bond Type with Nonmetal

Ionic bond (gaining electrons to form negative ions).

Bond Character (Electronegativity Diff 0.6)

Mostly covalent in character and formed between two nonmetals.

Bond Character (Electronegativity Diff 2.2)

Mostly ionic in character and formed between a metal and a nonmetal.

Gas Solubility vs Temperature

Solubility of gases decreases as temperature increases.

NaCl Saturated Solution (100C)

$40\,g$ dissolved in $100\,g\,H_2O$

KCl Saturated Solution (70C)

$46\,g$ dissolved in $100\,g\,H_2O$

Homogeneous Mixture Example

$$CO_2(aq)$$

Oxygen ppm Calculation

$4\,ppm$ for $0.040\,g$ oxygen in $10,000\,g$ solution.

KCl Solution Classification

Homogeneous mixture

Avogadro's Hypothesis Application

$3.0\,L$ of $N_2(g)$ contains the same number of molecules as $3.0\,L$ of $H_2(g)$ at STP.

Ideal Gas Behavior Conditions

High temperature and lower pressure.

Gas Volume Expansion Calculation

Increases from $2.0\,L$ to $2.5\,L$ when T increases to $30^{\circ}C$ and P decreases to $90\,kPa$.

CaO Electronegativity Difference

$$2.4$$

CaO Bond Type

Ionic

Melting Potential Energy Trend

Potential energy of the particles increases.

Gas Phase Particle Distance

Average distance between particles is greatest during the gaseous phase (Segment EF).

Homogeneous Mixture Distribution

Particles are distributed uniformly throughout the mixture.

NH4Cl Saturation (20g in 100g water @ 25C)

Unsaturated

$C_2H_4$ Structure

Ethene structural model

$CO_2$ Structure

Linear model (O=C=O)

Hydrogen Gas Structure

$H-H$ (Diatomic single bond)

Phenolphthalein Observation

Colorless in both acidic and neutral solutions.

Thomson's Atomic Particle Discovery

Electron

Rutherford's Atomic Structure Discovery

Nucleus

Group 2 Radius Trend Explanation

Atomic radius increases as you go down because more energy levels are added.

Group 2 Ion Charge

$$+2$$

CaO Compound Name

Calcium oxide

Synthesis Reaction

A reaction type like the production of CaO from Ca and O.

Group 2 Similarity Explanation

Atoms have the same number of valence electrons (two).

Evidence of Melting as Physical Change

Chemical composition remains the same (it is still chocolate).

Reason for Different Phases at Same Temp

Substances have different attractive forces or different melting points.

Allotropes definition

Different structural modifications of an element where atoms are bonded in a different manner.

Carbon Allotropes

Diamond, graphite, graphene, and fullerenes.

Heat of Fusion Segment

Segment BC on a heating curve.

Mole Ratio P4 to P2O5

1:2

Exothermic Reaction (P4 + O2)

A reaction that releases energy to the surroundings.

Freezing Point Identification

The temperature at which the cooling curve becomes horizontal between liquid and solid (e.g., $90^{\circ}C$).

Heat Released During DE (Hf Calculation)

$4830\,J$ for $20\,g$ of substance with $H_f = 241.5\,J/g$.

Solid Phase Duration (Cooling Curve)

2 minutes (from minute 14 to 16).

Atomic Count in 2H2O

6 atoms

Strontium Compound Highest % Sr

SrO

CaCrO4 % Oxygen by Mass

$$41\%$$

CH3CH2COOH Molecular Mass

$$74\,g/mol$$

Mass of 1.75 Moles NaSCN

$$141.75\,grams$$

Physical Property Example

Color

Stoichiometry: KClO3 to O2

$4\,moles$ of $KClO_3$ react to produce $6\,moles$ of $O_2$.

Empirical Formula Example

$$CH_4$$

Moles of Oxygen in 1 Mol N2O3

3

Lewis Dot Diagram LiCl

Li+ ion next to [Cl]- ion with 8 dots and brackets.