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View all PreK-12 NYS Learning Standards in a dropdown list format.
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  • Standard Area - TECH: Learning Standards for Technology
    (see MST standards under Previous Standard Versions)
          • Assessments
          • Assessments
            • Introduction - MST4.C.C.PS5.Introduction:

              Atoms and molecules are in constant motion. Chemical bonding between atoms involves energy and the interaction of electrons with atomic nuclei. Intermolecular attractions, which may be temporary, occur when there is an asymmetric distribution of charge.

              Within all chemical interactions, matter and energy are conserved according to the Law of Conservation of Matter and Energy. During a chemical change energy is absorbed or released as bonds are broken or formed. In maintaining conservation of matter and energy, nuclear changes convert matter into energy. The energy released during a nuclear change is much greater than the energy released during a chemical change.

              The discovery of the energy stored in the nucleus of an atom, its uses, and its inherent benefits and risks is a continuing process that began with the serendipitous detection of the first radioactive isotope. Early researchers added to this knowledge and expanded our ability to utilize this newly discovered phenomenon. Using radioactivity, the inner structure of the atom was defined by other researchers. Scientists involved in the development of nuclear fission and the atomic bomb explored both peaceful and destructive uses of nuclear energy. Modern researchers continue to search for ways in which the power of the nucleus can be used for the betterment of the world.

              Assessments
              • Major Understandings - MST4.C.C.PS5.2a:
                Chemical bonds are formed when valence electrons are: transferred from one atom to another (ionic), shared between atoms (covalent), and mobile within a metal (metallic)
                Assessments
              • Major Understandings - MST4.C.C.PS5.2b:
                Atoms attain a stable valence electron configuration by bonding with other atoms. Noble gases have stable valence configurations and tend not to bond.
                Assessments
              • Major Understandings - MST4.C.C.PS5.2c:
                When an atom gains one or more electrons, it becomes a negative ion and its radius increases. When an atom loses one or more electrons, it becomes a positive ion and its radius decreases.
                Assessments
              • Major Understandings - MST4.C.C.PS5.2d:
                Electron-dot diagrams (Lewis structures) can represent the valence electron arrangement in elements, compounds, and ions.
                Assessments
              • Major Understandings - MST4.C.C.PS5.2e:
                In a multiple covalent bond, more than one pair of electrons are shared between two atoms. Unsaturated organic compounds contain at least one double or triple bond.
              • Major Understandings - MST4.C.C.PS5.2f:
                Some elements exist in two or more forms in the same phase. These forms differ in their molecular or crystal structure, and hence in their properties.
                Assessments
              • Major Understandings - MST4.C.C.PS5.2g:
                Two major categories of compounds are ionic and molecular (covalent) compounds.
              • Major Understandings - MST4.C.C.PS5.2h:
                Metals tend to react with nonmetals to form ionic compounds. Nonmetals tend to react with other nonmetals to form molecular (covalent) compounds. Ionic compounds containing polyatomic ions have both ionic and covalent bonding.
              • Major Understandings - MST4.C.C.PS5.2i:
                When a bond is broken, energy is absorbed. When a bond is formed, energy is released.
                Assessments
              • Major Understandings - MST4.C.C.PS5.2j:
                Electronegativity indicates how strongly an atom of an element attracts electrons in a chemical bond. Electronegativity values are assigned according to arbitrary scales.
                Assessments
              • Major Understandings - MST4.C.C.PS5.2k:
                The electronegativity difference between two bonded atoms is used to assess the degree of polarity in the bond.
              • Major Understandings - MST4.C.C.PS5.2l:
                Molecular polarity can be determined by the shape of the molecule and distribution of charge. Symmetrical (non-polar) molecules include CO2, CH4, and diatomic elements. Asymmetrical (polar) molecules include HCl, NH3, and H2O.
                Educational Resources Assessments
              • Major Understandings - MST4.C.C.PS5.2m:
                Intermolecular forces created by the unequal distribution of charge result in varying degrees of attraction between molecules. Hydrogen bonding is an example of a strong intermolecular force.
                Assessments
              • Major Understandings - MST4.C.C.PS5.2n:
                Physical properties of substances can be explained in terms of chemical bonds and intermolecular forces. These properties include conductivity, malleability, solubility, hardness, melting point, and boiling point.
            • Educational Resources Assessments
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