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Test 3 chemistry
| Question | Answer |
|---|---|
| Describe Rutherford’s model of the atom | The atom has a tiny, dense, positively charged nucleus, Most of the atom is empty space, Electrons orbit the nucleus. Contains protons with +1 charge, and neutrons with no charge. |
| Define electromagnetic radiation | Electromagnetic radiation is energy that travels through space as waves made of oscillating electric and magnetic fields. |
| Define Electromagnetic radiation (continued...) | It doesn’t need a medium (it can travel through a vacuum), and it includes things like radio waves, microwaves, infrared, visible light, ultraviolet, X-rays, and gamma rays. |
| Explain how atoms emit light/energy/photons | Atoms emit light when their electrons are excited to higher energy levels and then fall back down, releasing the energy difference as photons. |
| Explain how the emission of spectrum of hydrogen demonstrates the quantized nature of energy | The hydrogen emission spectrum shows that electrons exist in fixed energy levels. When electrons are excited and then return to lower levels, they emit photons of specific energies, producing distinct lines and proving that atomic energy is quantized. |
| Describe the Bohr model of the atom | The Bohr model says electrons orbit the nucleus in fixed, quantized energy levels. They can jump between levels by absorbing or emitting photons of exact energy, explaining atomic spectra, while never spiraling into the nucleus. |
| List the features of the Wave Mechanical Model of the atom | The Wave Mechanical Model describes electrons as existing in orbitals or clouds, not fixed paths. It uses quantum mechanics to predict electron locations, includes energy quantization and spin, and explains atomic spectra and chemical behavior precisely. |
| Enumerate and describe the shapes of atomic orbitals | Atomic orbitals describe regions where electrons are likely found. s orbitals are spherical, p orbitals are dumbbell-shaped along axes, d orbitals are cloverleaf-shaped or donut-shaped, and f orbitals have complex multi-lobed shapes. |
| Determine and define the 4 periodic trends discussed in class | Atomic number counts protons. Ionization energy is the energy to remove electrons. Atomic radius is the distance to outer electrons. Metallic property shows how easily electrons are lost. Electronegativity measures attraction for bonding electrons. |
| Atomic Number trend | increases across each period (left to right) and down each group because you add one proton with each successive element. |
| Ionization Energy | generally increases across a period (electrons are held tighter by more protons) and decreases down a group (outer electrons are farther from the nucleus and easier to remove). |
| Atomic Radius | decreases across a period (more protons pull electrons in closer) and increases down a group (more electron shells are added). |
| Metallic Property | decreases across a period (atoms hold onto electrons more tightly) and increases down a group (atoms lose electrons more easily). |
| Electronegativity | increases across a period (atoms attract electrons more strongly) and decreases down a group (larger atoms attract electrons less effectively). |
| Differentiate ionic bond from covalent bond | An ionic bond occurs when one atom transfers electrons to another, forming positive and negative ions that attract each other, typically between a metal and a nonmetal. A covalent bond forms when atoms share electrons, usually between nonmetals. |
| Explain how the ionic bond and covalent bond are formed | An ionic bond forms when a metal atom loses electrons to become a positive ion and a nonmetal gains electrons to become a negative ion; the opposite charges attract. A covalent bond forms when two nonmetals share electrons to fill their outer shells. |
| Define polar bond and non-polar bond covalent bond | A polar covalent bond is formed when two atoms share electrons unequally, resulting in partial positive and negative charges because one atom pulls electrons more strongly, while a nonpolar covalent bond occurs when electrons are shared equally. |
| Determine polarity of a bond using electronegativity difference | To determine bond polarity, find the electronegativity difference between two atoms. If 0–0.4, the bond is nonpolar covalent; 0.5–1.7, it’s polar covalent with partial charges; greater than 1.7, it’s ionic, with electrons transferred to form ions. |
| Define electronegativity and its trend on the periodic table | Electronegativity is an atom’s ability to attract electrons in a bond. It increases across a period from left to right as atoms gain protons and decreases down a group as electrons are farther from the nucleus and less strongly attracted. |
| Define dipole moment | Property of a molecule whose charge distribution can be represented by a center of positive charge and a center of negative charge • Dipolar character of a molecule is represented by an arrow |
| Define octet rule and duet rule | The octet rule states that atoms tend to gain, lose, or share electrons to have eight electrons in their outermost shell for stability, while the duet rule applies to hydrogen and helium, which are stable with two electrons in their outer shell. |
| Define the VSEPR theory | VSEPR Theory (Valence Shell Electron Pair Repulsion) states that electron pairs around a central atom repel each other, so they arrange themselves as far apart as possible to minimize repulsion, determining the molecule’s shape. |
| Identify evidence for a chemical reaction | Any combination of color change, temperature change, gas, precipitate, or energy emission indicates a chemical reaction. |
Created by:
Masterlearner5