Section 1
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heterogeneous mixture
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Date created
Mar 1, 2020
Cards (60)
Section 1
(50 cards)
heterogeneous mixture
non-uniform
Complex Ionic Solids
have to contain at least one polyatomic ion
Pure Substance
cannot be separated by physical means
Isotopes
atoms of the same element that vary in the # of neutrons
Covalent Bond
- formed by sharing electrons, typically formed between 2 nonmetals (ex: CO2, HF, H2O)
Quarks
there are 6 identified quarks that make up protons and neutrons, named "up, down, top, bottom, strange & charm"
Classifying Bonds
- ionic (metal + nonmetal) - covalent (nonmetal+ nonmetal)
Mass Number
sum of protons and neutrons, must be a whole number
Ion
an atom or group of atoms that has a positive or negative charge, always formed by gaining or losing electrons
Polar Covalent
electrons are distributed asymmetrically (unevenly) around the molecule resulting in an unbalanced charge, result of the differing abilities for atoms to attract electrons
How are radioactive isotopes useful?
- studying the ratios of argon isotopes can provide insight into the origins and movement of magma and the ages of volcanic rock, Ar-40 begins increasing in concentration once lava has solidified - I-129 is a long-lived fission product that can be helpful in the detection of the movement of radiation after a radioactive event, in nuclear reactors and weapons tests, uranium and plutonium undergo fission processes where one of the products is I-129 which can be used as a groundwater tracer to determine evidence of nuclear fission and tracked in rainwater as evidence of fission event in air
Nuclear Decay
happens when there is a spontaneous transformation within the nucleus of an atom, changing one isotope to another isotope or even another element
Stable Isotopes
have no experimentally detected nuclear decays
Matter
Anything that has mass and takes up space
Nonpolar Covalent
electrons are distributed symmetrically (evenly) around the molecule resulting in a balanced charge
Colloid
a type of heterogeneous mixture in which particles of moderate size are suspended in a liquid, solid, or gas medium, exhibits the tyndall effect - scattering of light in a colloid (ex: fog, milk)
Mixture
can be separated by physical means, can be thought of as 2+ pure substances
Anion
a negative ion formed by gaining electrons
Atomic Mass of Element
the weighted average of the relative atomic masses of each pf the element's stable isotopes or long lived radioisotopes, taking into account each of their relative abundances
Fog
colloid
Intramolecular Forces
forces within a molecule, also called bonds, 2 main types: covalent and ionic
Why are radioisotopes usually not used to calculate atomic mass?
the relative abundance of a radioisotope will change as time passes, but if it has a very long half life, it is included if its relative abundance is large enough to contribute
Suspension
a type of heterogeneous mixture whose particles settle out over time and can be separated from the mixture by filtration (ex: ketchup, muddy water)
Electrons
one of six types of leptons, no structure, negatively charged
Chemical Formula
uses symbols and subscripts , states the number of atoms and of what kind
Salts
compounds that are held together by ionic bonds
Instantaneous Dipole - Induced Dipole (indip-indip) OR London Dispersion Forces (LDF)
- WEAK, only happens for an instant by random movement of electrons going towards one side (instantaneous dipole) repelling electrons on another molecule (inducing dipole on nonpolar adjacent molecule) - nonpolar, symmetrical - elements with more electrons have stronger LDFs bc they have more polarization - polymers can also form incredibly strong LDFs - ex: Helium, H2, CH4
Arsenic
element
Mass of Subatomic Particles
Proton has the most mass, Electrons have negligible mass, Neutrons weigh about the same as protons
Intermolecular Forces
forces that exist between molecules, indicated by dotted lines, what attracts one molecule to another molecule
Why is relative isotopic mass not a whole number?
- Protons and neutrons have different masses and different isotopes have different ratios of these particles - atomic masses are affected by binding energies (energy emitted when a nucleus is formed) --> e = mc^2 states that energy can be turned into mass and mass can be turned into energy - only exception is c-12
Simple Ionic Solids
just contain one metal and one nonmetal
Fresh squeezed lemonade
suspension
Ionic Bond
-formed by the attraction between oppositely charge ions -typically involves a metal and nonmetal
Electronegativity
the measure of the pull on electrons in a bond
Structural Formula
indicates the actual geometry of the molecules
Molecules
compounds held together by covalent bonds
Sand (SiO2)
compound
7-up
solution
Dipole - Dipole Force (dip-dip)
- STRONGER, more permanent than LDF - polar - negative side of polar molecules will attract to positive side of an adjacent polar molecules - ex: HCl, PH3, CH3Cl
Ice
compound
Atom C-12
serves as standard for the amu , is defined to have a mass of exactly 12 amu, all other atomic masses are measured relative to this
Radioisotopes
undergo nuclear decay (radioactive isotopes)
Half-life
amount of time it takes for half a sample of radioactive isotope to undergo a nuclear decay event (how radioactivity is measured)
Cation
a positive ion formed by losing electrons
Steel
solution
homogeneous
uniform (can apply to both mixtures - considered solutions and pure substances-elements, compounds)
Atomic Number
Indicates # of protons, identified the atom, for a neutral atom - # of protons = # of electrons
Bond
a force holding together the atoms in a compound
Atomic Mass of An Isotope
represents the mass of a specific isotope, also known as the relative isotopic mass, often given using the unit amu - atomic mass unit
Section 2
(10 cards)