front 1 What did De Broglie do? | back 1
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front 2 What is the Heisenberg Uncertainty Principle? | back 2
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front 3 What is Schrödinger’s model? | back 3 The quantum mechanical model of the atom comes from the solution to Schrödinger's equation. Provides the math for the quantization of electron energies. We assume that the location of the electron is probabilistic Thus:
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front 4 What is the Aufbau rule? | back 4 The Aufbau rule, or principle, states that electrons fill atomic orbitals from the lowest energy level to the highest. |
front 5 What is the Pauli Exlcusion principle | back 5 The Pauli Exclusion Principle states that no two identical fermions (like electrons) can occupy the same quantum state simultaneously. For electrons in an atom, this means a maximum of two electrons can be in the same orbital, and they must have opposite spins (one spin-up, one spin-down). This principle dictates how electrons fill atomic orbitals, which is the foundation for the structure of the periodic table. |
front 6 Which two elements are exceptions to Aufbau notation? | back 6 Cu, and Cr |
front 7 What is Hunds rule? | back 7 Fill the orbital levels by one before you double them up. |
front 8 What are Dalton's postualtes? | back 8 Dalton's atomic theory consists of five postulates: matter is made of indivisible atoms; all atoms of a given element are identical in mass and properties; atoms of different elements differ in mass and properties; atoms of different elements combine in simple, whole-number ratios to form compounds; and atoms are rearranged but not created or destroyed in chemical reactions. |
front 9 What are Thomson's discovery of electron properties? | back 9 Thomson's discovery of electron properties revealed that electrons are negatively charged subatomic particles with a mass much smaller than an atom's |
front 10 What was Rutherford's nuclear atom? | back 10 Rutherford's nuclear atom model describes an atom with a small, dense, positively charged nucleus at its center, which contains most of the atom's mass. Negatively charged electrons orbit this nucleus, with most of the atom being empty space. This model was proposed by Ernest Rutherford after his gold foil experiment, which showed that some alpha particles were deflected by a compact, central core, contradicting the earlier plum pudding model. |
front 11 Describe the structure of atoms and ions, including the masses, electrical charges, and locations of protons and neutrons in the nucleus and electrons in the electron cloud; | back 11 Atoms have a central, dense nucleus containing positively charged protons and neutral neutrons, which account for almost all the atom's mass. Negatively charged electrons are found in a surrounding electron cloud, and in a neutral atom, their number equals the number of protons. An ion is an atom that has gained or lost electrons, resulting in a net electrical charge because the number of protons and electrons is unequal. |
front 12 What are the properties of the alkali metals? | back 12 Alkali metals are shiny, soft, and highly reactive metals with low density and low melting points. They have one valence electron, which they readily lose to form a +1positive 1+1 cation, making them strong reducing agents. Their high reactivity means they must be stored under oil to prevent reaction with air and are never found freely in nature. |
front 13 What are the properties of the alkali earth metals? | back 13 Alkali earth metals are shiny, silvery-white metals that are relatively soft, have low densities, and are good conductors of heat and electricity. Their key properties include having two electrons in their outermost shell, which makes them highly reactive (though less so than alkali metals) and gives them a 2+2 plus2+ oxidation state. They are found in compounds in nature because of this reactivity. +2 ions |
front 14 What are the halogens properties? | back 14 Halogens are a group of highly reactive, non-metal elements in Group 17 of the periodic table. Their key properties include having seven valence electrons, which makes them highly electronegative and prone to gaining one electron to form a stable ion with a -1negative 1−1 charge. As you move down the group, reactivity decreases, but melting and boiling points increase. They exist in all three states of matter at room temperature: fluorine and chlorine are gases, bromine is a liquid, and iodine and astatine are solids. -1 ions |
front 15 What are the properties of the noble gases. | back 15 Noble gases are a group of colorless, odorless, non-flammable, and largely unreactive monatomic gases with low boiling points. Their inertness stems from having a full outer shell of valence electrons, making them chemically stable. They exist as individual atoms rather than molecules, and when subjected to electricity at low pressure, they glow, which is used in applications like lighting. They're in group 18. |
front 16 What are the properties of transition metals? | back 16 Transition metals are hard, shiny metals that are good conductors of heat and electricity, have high melting and boiling points, and are malleable and ductile. They are also characterized by their ability to form colored compounds, form complexes, and exhibit multiple oxidation states due to their partially filled d orbitals. |
front 17 What is the atomic radius? | back 17 <-------------------------------------------------- | | | ↓ |
front 18 What are metals? | back 18
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front 19 What are metalloids? | back 19
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front 20 What are non metals | back 20
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front 21 Whats the difference between Mendeleev and Moselys periodic table? | back 21 The main difference is that Mendeleev arranged elements by increasing atomic mass, while Moseley arranged them by increasing atomic number. This change, based on Moseley's discovery of a more fundamental property, resolved inconsistencies in Mendeleev's table, such as the placement of elements like iodine and tellurium, and laid the foundation for the modern periodic table. |
front 22 What do the arrows for electronegativity look like? | back 22 Up right Right, relative ability of an atom to attract electrons while in a bond. |
front 23 What do the arrows for ionization energy and electron affinity look like? | back 23 Right to up, the amount of energy required to remove an electron from an atom. |
front 24 What do the arrows Nonmetallic and metallic properties looks like? | back 24 Cross body |
front 25 What is effective nuclear charge? | back 25 The amount of attraction the valence electrons have to the nucleus. Right down |
front 26 What is the shielding effect? | back 26 The higher amount of orbitals the greater the shielding effect ie less nuclear charge ie bigger atomic radius. |
front 27 What is an anion? | back 27 More electron than protons, greater e cloud size |
front 28 What is a cation? | back 28 Less electrons than protons, lesser e cloud size |
front 29 When a neutral atom becomes a negatively charge ion how an why does the size change. | back 29 It becomes bigger because there's more electron-electorn repulsion. |
front 30 How many electrons fit into the different blocks: S, P, D, F | back 30 2, 6, 10, 14 respectively |
front 31 What does e - mean? | back 31 Losing one orbital |
front 32 What is a chemical family? | back 32 A chemical family is a group of elements in the periodic table that share similar properties due to having the same number of valence electrons. |
front 33 What is a chemical period? | back 33 A horizontal row of elements |