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EmSAT Achieve Physics and Chemistry Core Concepts

25 flashcards reviewing essential physics formulas, mechanics principles, chemical bonding, and reaction thermodynamics for EmSAT Achieve.

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Newton's Second Law of Motion
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1
Newton's Second Law of Motion
F_net = m * a; net force equals mass multiplied by acceleration, measured in Newtons (N).
2
Translational Kinetic Energy Formula
KE = 0.5 m v^2; scalar energy of an object of mass m moving with linear velocity v.
3
Gravitational Potential Energy (Uniform Field)
PE = m g h; energy stored by elevating an object of mass m to height h in gravitational field g.
4
Work-Energy Theorem
W_net = Delta KE; total net work performed on a particle equals the resulting change in its kinetic energy.
5
Linear Momentum and Impulse Relationship
p = m v; Impulse J = Delta p = F_avg Delta t, representing change in linear momentum over time interval Delta t.
6
Hooke's Law for Ideal Springs
F_s = -k * x; restoring spring force directed opposite to displacement x with spring stiffness constant k.
7
Ohm's Law for Ohmic Conductors
V = I * R; electrical potential difference equals electric current I multiplied by resistance R.
8
Electrical Power Dissipation Formulas
P = V I = I^2 R = V^2 / R; rate of electrical energy transfer expressed in Watts (W).
9
Coulomb's Law of Electrostatic Force
F_e = k_e |q1 q2| / r^2; magnitude of electrostatic force between two point charges separated by distance r.
10
Snell's Law of Refraction
n1 sin(theta1) = n2 sin(theta2); relates indices of refraction and angles of propagation at a boundary.
11
Universal Wave Equation
v = f * lambda; propagation speed of a periodic wave equals frequency f multiplied by wavelength lambda.
12
Ideal Gas Law Equation of State
P V = n R * T; relates absolute pressure P, volume V, moles n, ideal gas constant R, and Kelvin temperature T.
13
Avogadro's Constant Definition
N_A approximately 6.022 * 10^23 particles/mol; number of constitutive units (atoms, molecules) in one mole.
14
Molarity (Molar Concentration)
M = n_solute / V_solution (in liters); concentration expressing moles of dissolved solute per liter of total solution.
15
Definition of pH Scale
pH = -log10[H+]; logarithmic index quantifying hydrogen ion (hydronium) activity in an aqueous solution.
16
Arrhenius Acid-Base Neutralization
Acid + Base -> Salt + Water; classic neutralization forming an ionic compound and water.
17
Exothermic vs. Endothermic Enthalpy Changes
Exothermic processes release thermal energy (Delta H < 0); endothermic processes absorb heat (Delta H > 0).
18
Le Chatelier's Principle
When a chemical system in dynamic equilibrium experiences a stress, it shifts in the direction that counteracts the stress.
19
Hess's Law of Constant Heat Summation
Total enthalpy change Delta H for a chemical reaction is independent of the pathway and equals the sum of step enthalpies.
20
Covalent vs. Ionic Chemical Bonding
Covalent bonds involve mutual electron-pair sharing between nonmetals; ionic bonds involve electrostatic transfer.
21
Periodic Trend: Electronegativity
Atom's relative ability to attract shared electrons; increases from left to right across periods, decreases down groups.
22
First Law of Thermodynamics
Delta U = Q - W; change in system internal energy equals heat added to system minus mechanical work done by system.
23
Specific Heat Capacity Equation
Q = m c Delta T; heat energy Q required to change the temperature of mass m of specific heat capacity c by Delta T.
24
Boyle's Law for Ideal Gases
P1 V1 = P2 V2; pressure and volume are inversely proportional at fixed temperature and constant mole amount.
25
Charles's Law for Ideal Gases
V1 / T1 = V2 / T2; gas volume is directly proportional to absolute Kelvin temperature at constant pressure.

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