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Chemistry210 Exam 1
Chemistry210 Exam study cards for KSU
| Question | Answer |
|---|---|
| What is an Anion | Negative charged atom that gains one or more electrons |
| What is a Cation | Positive charged atom that loses one or more electrons |
| What is the atomic number, and the abbreviation for it? | The number of protons (z) |
| What is the mass number, and the abbreviation for it? | Number of protons plus the number of neutrons (A) |
| How do you find the number of neutrons? | Mass number - Atomic number (A-Z) |
| What's an Isotope? | Atoms of the same atomic number (Z) but different mass number (A). Most elements have 2+ isotopes |
| How do you find the average mass? | Isotopic mass X fractional abundance. |
| Which groups are in the S subshell? | 1A and 2A and Helium |
| Which groups are in the D subshell? | 1B through 7B and 8 |
| Which groups are in the F subshell? | Lanthanides and Actinides? |
| Which groups are in the P subshell? | 3A to 8A minus Helium |
| Atomic radius decreases as you go.. | Right and Down |
| What is the alpha particle? | Positive particle with two protons and two neutrons. |
| What is Dalton? | Alternative unit equivalent to the atomic mass unit. |
| What is Dalton's atomic theory? | Set of postulates that established the fundamental properties of atoms |
| What is the empirical formula? | formula showing the composition of a compound given as the simplest whole-number ratio of atoms |
| What is the fundamental unit of charge? | (also called the elementary charge) equals the magnitude of the charge of an electron (e) with e = 1.602 × 10−19 C |
| What is an Ion? | electrically charged atom or molecule (contains unequal numbers of protons and electrons) |
| What is an isomer? | compounds with the same chemical formula but different structures |
| What is the law of constant composition? | (also, law of definite proportions) all samples of a pure compound contain the same elements in the same proportions by mass. |
| What is the law of definite proportions? | (also, law of constant composition) all samples of a pure compound contain the same elements in the same proportions by mass |
| what is the law of multiple proportions? | when two elements react to form more than one compound, a fixed mass of one element will react with masses of the other element in a ratio of small whole numbers |
| What is the molecular formula? | formula indicating the composition of a molecule of a compound and giving the actual number of atoms of each element in a molecule of the compound. |
| What are spatial isomers? | compounds in which the relative orientations of the atoms in space differ |
| What is the structural formula? | shows the atoms in a molecule and how they are connected |
| What is a structural isomer? | one of two substances that have the same molecular formula but different physical and chemical properties because their atoms are bonded differently |
| What is an Actinide? | inner transition metal in the bottom of the bottom two rows of the periodic table |
| What is an Alkali Metal? | Element in group 1A |
| What is an Alkaline earth metal? | Element in group 2A |
| What is amplitude? | extent of the displacement caused by a wave |
| What is the atomic orbital? | mathematical function that describes the behavior of an electron in an atom (also called the wavefunction) |
| What is the Aufbau Principle? | It states that electrons fill lower energy orbit before filling the higher ones. |
| What is a blackbody? | idealized perfect absorber of all incident electromagnetic radiation; such bodies emit electromagnetic radiation in characteristic continuous spectra called blackbody radiation |
| What is Bohrs model of the hydrogen atom? | structural model in which an electron moves around the nucleus only in circular orbits, each with a specific allowed radius |
| What is a chalcogen? | Element in group 6A |
| What is the continuous spectrum? | electromagnetic radiation given off in an unbroken series of wavelengths (e.g., white light from the sun) |
| What is the core electron? | electron in an atom that occupies the orbitals of the inner shells covalent bond |
| What is a covalent bond? | (also, molecular compound) composed of molecules formed by atoms of two or more different elements |
| What is a covalent radius? | one-half the distance between the nuclei of two identical atoms when they are joined by a covalent bond |
| What is the D orbital? | region of space with high electron density that is either four lobed or contains a dumbbell and torus shape; describes orbitals with l = 2. |
| What are degenerate orbitals? | orbitals that have the same energy |
| What is an affective nuclear charge? | charge that leads to the Coulomb force exerted by the nucleus on an electron, calculated as the nuclear charge minus shielding |
| What is electromagnetic radiation? | energy transmitted by waves that have an electric-field component and a magnetic-field component |
| What is the electromagnetic spectrum? | range of energies that electromagnetic radiation can comprise, including Gamma, X-ray, UV, Infrared, Microwave, Broadcast, and Wireless radio lights. |
| What is the electron affinity? | energy change associated with addition of an electron to a gaseous atom or ion |
| What is the electron configuration? | listing that identifies the electron occupancy of an atom’s shells and subshells |
| What is the electron density? | a measure of the probability of locating an electron in a particular region of space, it is equal to the squared absolute value of the wave function ψ |
| What does endothermic mean? | processes that increase the energy of an atom and involve the absorption of light |
| what does an excited state mean? | state having an energy greater than the ground-state energy |
| what does exothermic mean? | processes that decrease the energy of an atom and involve the emission of light |
| What is the F orbital? | multilobed region of space with high electron density, describes orbitals with l = 3 |
| What is the frequency (v) | number of wave cycles (peaks or troughs) that pass a specified point in space per unit time |
| What does ground state mean? | state in which the electrons in an atom, ion, or molecule have the lowest energy possible |
| What group are halogens in? | Group 7A |
| What is the Heisenburg uncertainty principle? | It states that we cannot know both the speed and position of a particle (such as a photon or electron) with perfect accuracy |
| What are Hertz? | The unit of frequency, the number of cycles per second (S -1) |
| What is Hunds Role? | every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin inert gas |
| What is an inert gas? | (AKA Noble Gas) in group 8A |
| What is an inner transition metal? | (also, lanthanide or actinide) element in the bottom two rows; if in the first row, also called lanthanide, or if in the second row, also called actinide |
| What does intensity mean? | property of wave-propagated energy related to the amplitude of the wave, such as brightness of light or loudness of sound |
| What is an interference pattern? | pattern typically consisting of alternating bright and dark fringes; it results from constructive and destructive interference of waves |
| What is an ionic bond? | electrostatic forces of attraction between the oppositely charged ions of an ionic compound |
| What is an ionic compound? | compound composed of cations and anions combined in ratios, yielding an electrically neutral substance |
| What is ionization energy? | energy required to remove an electron from a gaseous atom or ion |
| What does isoelectronic mean? | group of ions or atoms that have identical electron configurations |
| What is the line spectrum? | electromagnetic radiation emitted at discrete wavelengths by a specific atom (or atoms) in an excited state magnetic quantum number (ml) |
| Which groups are the "Main group element"? | (AKA representative element) element in groups 1A, 2A, 3A-8A |
| What is a metal? | element that is shiny, malleable, good conductor of heat and electricity |
| What is a mettaloid? | element that conducts heat and electricity moderately well, and possesses some properties of metals and some properties of nonmetals |
| What is a molecular compound? | (also, covalent compound) composed of molecules formed by atoms of two or more different elements |
| What is a monoatomic Ion? | ion composed of a single atom. |
| What is a Noble gas? | (AKA inert gas) element in group 8A |
| What is a node? | any point of a standing wave with zero amplitude |
| What is a nonmetal? | element that appears dull, poor conductor of heat and electricity |
| What is an orbital diagram? | pictorial representation of the electron configuration showing each orbital as a box and each electron as an arrow |
| What is an oxyanion | polyatomic anion composed of a central atom bonded to oxygen atoms |
| What is a P orbital? | dumbbell-shaped region of space with high electron density, describes orbitals with l = 1 |
| What is the Pauli exclusion principle? | specifies that no two electrons in an atom can have the same value for all four quantum numbers |
| What is the periodic law? | properties of the elements are periodic function of their atomic numbers |
| What is the periodic table? | table of the elements that places elements with similar chemical properties close together |
| What is a photon? | smallest possible packet of electromagnetic radiation, a particle of light |
| What is a pnictogen? | Element in group 5A |
| What is a polyatomic ion? | Ion composed of more than one atom |
| What are the principle quantum numbers? (n) | quantum number specifying the shell an electron occupies in an atom |
| What does quantization mean? | limitation of some property to specific discrete values, not continuous |
| What are quantum mechanics? | field of study that includes quantization of energy, wave-particle duality, and the Heisenberg uncertainty principle to describe matter |
| What is the S orbital? | spherical region of space with high electron density, describes orbitals with l = 0 |
| What is the secondary (angle momentum) quantum number? | (l), quantum number distinguishing the different shapes of orbitals; it is also a measure of the orbital angular momentum |
| What is the spin quantum number? | (Ms), number specifying the electron spin direction, either +1/2 or −1/2 |
| What is a standing wave? | (also, stationary wave) localized wave phenomenon characterized by discrete wavelengths determined by the boundary conditions used to generate the waves; standing waves are inherently quantized |
| What is a subshell? | atomic orbitals with the same values of n and l |
| What is a transition metal? | element in groups 3–12 (more strictly defined, 3–11; see chapter on transition metals and coordination chemistry) |
| What are valence electrons? | electrons in the high energy outer shell(s) of an atom |
| What is a valence shell? | high energy outer shell(s) of an atom |
| What is a wave? | oscillation of a property over time or space; can transport energy from one point to another |
| What is wave particle duality | observation that elementary particles can exhibit both wave-like and particle-like properties |
| What is the wavefunction (ψ) | describes the shape of the orbital; it can be used to calculate the probability of finding the electron at any given location in the orbital, as well as dynamical variables such as the energy and the angular momentum |
| What is the wavelength (λ) | distance between two consecutive peaks or troughs in a wave |
| What do subscripts show? | the actual number of atoms of each type in the molecule |
| What is Avogadros number? | 6.02x10^23 |
| What is a mole? | Amount unit similar to familiar units like pair or dozen |
| How do you find the number of atoms? | Avogadro's number x #moles of atoms |
| How do you find the number of molecules? | Avogadro's number x #moles of molecules |
| How do you find the number of moles for an atom? | #atoms divided by avogadros number |
| How do you find the number of moles for a molecule? | #molecules divided by avogadros number |
| What are the molar mass formulas? | #moles=mass/molar mass molar massX#moles=mass |
| Symbol for speed of light? | c |
| Symbol for wavelength? | lambda |
| Symbol for frequency? | V |
| Symbol for Planck's constant? | h 6.63x10^-34 |
| Formula for finding the speed of light? | C=(lambda)x(v) |
| Formula for finding energy? | E=hv OR E=h(c/lambda) |
| In the electromagnetic spectrum, Gamma has what? | The shortest wavelength, the highest frequency, and the highest energy. |
| What are all waves characterized by? | Wavelength, frequency, and amplitude |
| What is the classical wave theory? | A wave's energy depends on its intensity not frequency |
| Formula for finding wavelength? | Lambda=h/mu |
| symbol for velocity? | u |
| The rules for the quantum numbers? | n=1,2,3,..... l = (n-1) plus anything lower than that above -1 ml = -l to +l ms = +1/2 -1/2 |
| What does paramagnetic mean? | When there are one or more unpaired electrons |
| What does diamagnetic mean? | When all of the electrons are paired in an atom |
| Are cations with a larger charge smaller or larger than cations with a smaller charge? | Smaller |
| Are anions larger or smaller than the atom it is derived from? | larger |
| What does a larger radius signify? | It shows the atom has more electrons that are repelling each other. |
| What does isoelectronic mean? | Atoms and ions that have the same electron configuration. Which means the greater the nuclear charge, the smaller the radius in a series of isolectronic ions and atoms. |
| Is energy always required to remove electrons? | Yes |
| What decreases with the increase of the atomic radius? | Ionization energy |
| How do ionization energies decrease/increase on a periodic table? | Decreases down a group, increases across a period |
| What is the electron affinity? | (EA) the energy change for the process of adding an electron to a gaseous atom to form an anion |
| What does a negative EA mean? | energy is released |
| What is the first ionization energy? | Energy that's absorbed when an electron is removed from an atom in the gas phase. As atomic radius increases across a period, it becomes easier to remove an electron and the ionization energy should decrease. Noble gases have the highest |
| What does the first electron affinity mean? | Energy is released when an atom in the gas phase gains an electron. As the nuclear charge of atoms increases it becomes easier to add an electron and the EA becomes more negative. Halogens have the highest. |
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