New York State Regents Examinations Physical Setting / Chemistry (Regents Examination) Syllabus

Physical Setting / Chemistry (Regents Examination) syllabus — full chapter and topic list

Expand any chapter to see its topics and sub-topics. This is the whole examinable outline for Physical Setting / Chemistry (Regents Examination) in New York State Regents Examinations, not a summary of it.

1. 1

   Atomic Structure and the Periodic Table

   3 topics

   • Models of the Atom
     • Subatomic particles and atomic number/mass
     • Electron configuration and energy levels
   • Isotopes and Atomic Mass
     • Calculating average atomic mass
   • Periodic Trends
     • Groups, periods, and reactivity
     • Atomic radius, ionization energy, electronegativity
2. 2

   Bonding and Chemical Formulas

   3 topics

   • Types of Chemical Bonds
     • Ionic, covalent, and metallic bonding
     • Polarity and intermolecular forces
   • Naming and Writing Formulas
     • Nomenclature of compounds and polyatomic ions
   • Molecular Geometry and Properties
     • Relating structure to physical properties
3. 3

   Stoichiometry and Chemical Reactions

   3 topics

   • The Mole and Formula Mass
     • Mole conversions and percent composition
   • Balancing Chemical Equations
     • Conservation of mass and reaction types
   • Mole-Ratio Calculations
     • Using coefficients in proportions
4. 4

   Physical Behavior of Matter

   3 topics

   • States of Matter and Phase Change
     • Kinetic molecular theory
     • Heating and cooling curves
   • The Gas Laws
     • Relationships among pressure, volume, and temperature
     • Combined gas law calculations
   • Solutions and Mixtures
     • Solubility and concentration (molarity, ppm)
     • Effects on boiling and freezing points
5. 5

   Energy, Kinetics, and Equilibrium

   3 topics

   • Thermochemistry
     • Endothermic and exothermic reactions
     • Calorimetry and heat calculations
   • Reaction Rates and Equilibrium
     • Factors affecting reaction rate
     • Le Chatelier's principle
   • Entropy and Spontaneity
     • Tendency toward lower energy and higher entropy
6. 6

   Acids, Bases, Redox, Organic, and Nuclear Chemistry

   4 topics

   • Acids and Bases
     • pH scale and indicators
     • Neutralization and titration
   • Oxidation-Reduction and Electrochemistry
     • Oxidation numbers and half-reactions
     • Voltaic and electrolytic cells
   • Organic Chemistry
     • Hydrocarbons and functional groups
     • Organic reactions (substitution, addition, esterification)
   • Nuclear Chemistry
     • Radioactive decay and half-life
     • Fission, fusion, and applications

Physical Setting / Chemistry (Regents Examination) flashcards for New York State Regents Examinations

21 of 74 cards from the Physical Setting / Chemistry (Regents Examination) deck — real questions with worked answers.

1. What are the three subatomic particles, and what is the charge and relative mass of each?

   Protons (+1 charge, ~1 amu) and neutrons (0 charge, ~1 amu) are in the nucleus; electrons (-1 charge, ~1/1836 amu, essentially 0) occupy the surrounding orbitals.

2. How did the gold-foil (Rutherford) experiment change the model of the atom?

   Most alpha particles passed straight through, but a few deflected sharply, showing the atom is mostly empty space with a small, dense, positively charged nucleus rather than a uniform 'plum pudding' of charge.

3. In the wave-mechanical (modern) model of the atom, what is an orbital?

   A region of space around the nucleus where there is a high probability of finding an electron; electrons are described by probability clouds rather than fixed circular paths.

4. What is an excited state of an atom, and what happens when an electron returns to the ground state?

   An excited state is when an electron has absorbed energy and jumped to a higher energy level. When it falls back to a lower level (ground state), it releases a specific amount of energy as a photon of light, producing the element's bright-line spectrum.

5. What are isotopes?

   Atoms of the same element (same number of protons) that have different numbers of neutrons, and therefore different mass numbers.

6. How is the atomic mass of an element on the periodic table calculated?

   It is the weighted average of the masses of all naturally occurring isotopes: multiply each isotope's mass by its decimal abundance and add the results.

7. How do you determine the number of neutrons in an atom or isotope?

   Subtract the atomic number (number of protons) from the mass number (protons + neutrons): neutrons = mass number − atomic number.

8. Calculate the average atomic mass of an element with two isotopes: mass 10 amu at 20% abundance and mass 11 amu at 80% abundance.

   (10 × 0.20) + (11 × 0.80) = 2.0 + 8.8 = 10.8 amu.

9. How do atomic radius, ionization energy, and electronegativity change across a period (left to right)?

   Atomic radius decreases, while ionization energy and electronegativity increase across a period from left to right.

10. How do atomic radius, ionization energy, and electronegativity change down a group?

    Atomic radius increases, while ionization energy and electronegativity decrease going down a group.

11. Why does atomic radius decrease across a period?

    As protons are added across a period, the increasing nuclear charge pulls the electrons (in the same principal energy level) more tightly toward the nucleus, shrinking the atom.

12. How does the radius of a positive ion (cation) compare to its neutral atom, and a negative ion (anion) to its neutral atom?

    A cation is smaller than its neutral atom (it loses electrons/an energy level); an anion is larger than its neutral atom (added electrons increase electron-electron repulsion).

13. What is the difference between a metal and a nonmetal in terms of electron behavior and properties?

    Metals tend to lose electrons (low ionization energy), are good conductors, malleable, and lustrous; nonmetals tend to gain electrons (high electronegativity), are poor conductors, and brittle as solids.

14. What is an ionic bond and between what types of elements does it typically form?

    An ionic bond is the electrostatic attraction between oppositely charged ions formed by the transfer of electrons, typically between a metal and a nonmetal.

15. What is a covalent bond, and what is the difference between a polar and a nonpolar covalent bond?

    A covalent bond is the sharing of electrons between nonmetal atoms. It is nonpolar when electrons are shared equally (small/zero electronegativity difference) and polar when shared unequally (greater electronegativity difference).

16. What is metallic bonding?

    Bonding in metals described as positive metal ions (kernels) immersed in a 'sea' of mobile, freely moving valence electrons, which accounts for conductivity and malleability.

17. How can the electronegativity difference between two atoms be used to predict bond type?

    A large difference (roughly ≥1.7) indicates an ionic bond; a small-to-moderate difference indicates polar covalent; a difference near zero indicates nonpolar covalent.

18. Why do ionic compounds conduct electricity when melted or dissolved but not as solids?

    In the solid the ions are locked in a fixed crystal lattice, but when melted or dissolved the ions become mobile and free to carry charge.

19. What is the rule for naming a binary ionic compound (metal + nonmetal)?

    Name the metal (cation) first, then the nonmetal with its ending changed to -ide (e.g., NaCl = sodium chloride). Use Stock notation (Roman numerals) for the charge of multivalent metals (e.g., FeCl3 = iron(III) chloride).

20. What prefixes are used in naming molecular (covalent) compounds, and what is CO2 named?

    Prefixes indicate the number of atoms: mono-(1), di-(2), tri-(3), tetra-(4), penta-(5). CO2 is carbon dioxide (mono- is omitted on the first element).

21. Write the correct formula for aluminum oxide using oxidation numbers.

    Al is +3 and O is -2; crossing charges gives Al2O3.

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