CHEM 1011 - Lecture Notes 9_6_23

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Atoms are the smallest constituent of matter that retains chemical behavior (i.e. form chemical bonds). Elements are substances that cannot be broken down further by any chemical means. Elements can exist in the solid, liquid, or gas phase. The electron cloud surrounds the nucleus of an atom. - Surround nucleus with probability density (“orbital”) - Makes chemical bonds - Negatively charged and very low density The periodic table: An organized array of chemical elements based on common properties ● Periods - Horizontal rows; systematics in electron distribution ● Groups - Vertical columns; similarities in chemical reactivity ● Group 1: Alkali metals ● Group 2: Alkaline earths ● Groups 3-12: transition metals ● Gorup 17: Halogens ● Group 18: Noble gases The periodic table: metals, metalloids, and nonmetals ● Metals ○ Malleable - you can hammer it down in sheets ○ Ductile ○ Conductors ○ > 75% of p table ● Metalloids - b/w metals and nonmetals; brittle, semiconductors, dopants ● Nonmetals - Poor conductors, dull, brittle solids or gases Atomically precise compositions are denoted with chemical symbols. Not all atoms have the same number of subatomic particles: Ions and isotopes Ions are atoms with a net electrical charge (imbalance in number of protons and electrons Z = #p+ - #e- Cation = net positive charge Anion = net negative charge Isotopes are atoms (or ions) of the same elements with differing numbers of neutrons .
Fluorine-18 has 9 protons, 9 neutrons, and 9 electrons. It is used in PET scans to detect cancer and tumor cells. Fluorine-19 has 9 protons, 10 neutrons, and 9 electrons → inert How do we relate atomic composition to its mass? ● Matter contains mass and mass is the amount of stuff something has ● For atoms, that amount of stuff is the number of protons, neutrons and electrons ○ Proton - p+ → mass = 1.67262 x 10^-27 kg → relative charge +1 ○ Neutron - n0 → mass = 1.67493 x 10^-27 kg → relative charge 0 ○ Electron - e- → mass = 9.109 x 10^-31 kg → relative charge -1 From this → Atomic masses ≈ 10^-26kg We can define a convenient unit where we drop the 10^-26 We just need a reference! In AMU (atomic mass unit), atomic masses are very close to mass number. Masses reported on periodic table are not for pure isotopes. - Elements commonly occur as mixtures of isotopes. - The atomic mass number in the periodic table is actually the weighted average of isotope masses; - Isotopes are weighted by relative abundance
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