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CHEMISTRY - Coggle Diagram
CHEMISTRY
CHEMICAL BONDS
Chemical bonds- an attraction between two atoms, resulting from a sharing of outer-shell electrons or the presence of opposite charges on atoms. The bonded atoms gain complete outer electron shells
Covalent bonds type of strong chemical bond in which two atoms share one or more pairs of valence electrons
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nonpolar covalent bond- covalent bond in which electrons are shared equally between two atoms of similar electronegativity
Polar covalent bond- covalent bond between atoms that differ in electronegativity, the shared electrons are pulled closer to the more electronegative atom, making one slightly negative atom and slightly positive atom
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Hydrogen bond- noncovalent attraction between a hydrogen and an electronegative atom, a weak bond
ELEMENTS AND COMPOUNDS
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Emergent Properties- characteristics that arise from the arrangement and interaction of parts within a system, but are not present in the individual components themselves
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Essential elements - a chemical element required for an organism to survive, grow, and reproduce
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CHEMICAL REACTIONS
Chemical reactions- making and breaking of chemical bonds, leading to changes in the composition of matter
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Reactions cannot create or destroy atoms, but can only rearrange the electrons among them
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Chemical equilibrium- in a chemical reaction, the state in which the rate of the forward reaction equals the rate of the reverse reaction
STRUCTURE OF ATOMS
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Subatomic particles- the smaller components that make up an atom; there are 3 primary subatomic particles
Protons carry a positive charge and are found in the nucleus of an atom. The number of protons defines the atomic number of an element
Neutrons do not have a charge; they are neutral. They are also located in the nucleus alongside protons.
Electrons are negatively charged particles that orbit the nucleus in a cloud-like formation. Their movement and energy levels are crucial to chemical reactions
Atomic nucleus- an atom's dense central core, containing protons and neutrons
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ISOTOPES
Isotopes- atomic form of an element, each with the same number of protons but a different number of neutrons, thus differing in atomic mass
Example of an isotope would be Carbon 12, Carbon 13, and Carbon 14. They all have 6 protons, but C12 has 6 neutrons, C13 has 7 neutrons, and C14 has 8 neutrons
Radioactive isotope - one in which the nucleus decays spontaneously, giving off particles and energy. When radioactive decay leads to a change in the number of protons, it turns an atom into an atom of a different element
An example of a radioactive isotope is when a carbon-14 atom decays, a neutron decays into a proton, reverting to nitrogen
Half-life-the amount of time it takes for half of a sample of a radioactive isotope to decay. Values range from seconds to thousands of years.
radiometric dating-method for determining the age of rocks and fossils, based on the half-life of radioactive isotopes
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