Chapters 1 (Intro to Chemistry) and 2 (Matter and Change)

Chemistry Learning Targets (Chemistry A)

Chapters 1 (Intro to Chemistry) and 2 (Matter and Change)

HSCE / Target/s:
I can statements. / Give an example that demonstrates your knowledge of the target or explain the target in your own words.
C1.1A / I can generate a new question that could be investigated in a lab.
C1.1B / I can identify possible sources of error in an experiment.
C1.1B / I can evaluate the validity of scientific conclusions.
C1.1C / I can conduct a scientific investigation using the appropriate instrument/tool.
C1.1D / I can identify patterns in data.
C1.1D / I can relate patterns in data to theoretical models.
P3.p1A / I can relate the amount of energy needed to heat a substance to the amount of energy released by a substance.
C3.4A / I can use the term endothermic to describe a chemical reaction
C3.4A / I can use the term exothermic to describe a chemical reaction.
P4.p2A / I can make a drawing to show the difference between an element, compound and mixture.
P4.p2B / I can use physical properties to identify a pure substance (element or compound.)
P4.p2C / I can separate mixtures based on the physical properties of the individual components.
P4.p2D / I can recognize that there are differences between properties of an element and the compounds in which those elements are found.

Chapter 3: Scientific Measurement

HSCE / Target/s:
I can statements. / Give an example that demonstrates your knowledge of the target or explain the target in your own words.
I can convert measurements to scientific notation.
I can distinguish among accuracy, precision, and error or measurement.
I can distinguish the number of significant figures in a measurement and in a calculated answer.
I can list SI units of measurement and common SI prefixes.
I can distinguish between the mass and weight of an object.
I can construct conversion factors from equivalent measurements.
I can apply the technique of dimensional analysis to a variety of conversion problems.
I can solve problems by breaking the solution into steps.
I can convert complex units, using dimensional analysis.
I can calculate the density using experimental data.
I can describe how density varies with temperature.

Chapters: 4 (Atomic Structure), 5 (Electrons in Atoms) and 6 (The Periodic Table)

HSCE / Target/s:
I can statements. / Give an example that demonstrates your knowledge of the target or explain the target in your own words.
C4.8A / I can identify the location, relative mass, and charge for electrons, protons and neutrons.
C4.8B / I can accurately describe an atom based on the most current model (electron cloud).
C4.8C / I can describe how the strong force on a nucleus helps to keep it intact.
C4.8D and C4.10A / I can list the number of protons, neutrons and electrons for any ion or isotope (for example: fluoride ion with a -1 charge).
C4.10B / I can recognize that an element always has the same number of protons.
C4.10c / I can calculate the average atomic mass of an element given the percent abundance and mass of the individual isotopes.
C4.10d / I can predict which isotope will have the greatest abundance given the possible isotopes for an element and the average atomic mass in the periodic table.
C4.10e / I can write the symbol for an isotope, ZA X where Z is the atomic number, A is the mass number, and X is the symbol for the element.
C2.4a / I can describe energy changes in flame tests of common elements in terms of the electron transitions.
C2.4b / I can contrast the mechanism of energy changes and the appearance of absorption and emission spectra.
C2.4c / I can explain why an atom can only absorb certain wavelengths of light.
C2.4d / I can compare various wavelengths of light (visible and nonvisible) in terms of frequency and relative energy.
C4.8e / I can write the complete electron configuration of elements in the first four rows of the periodic table.
C4.8f / I can write kernel structures for main group elements.
C4.8g / I can predict oxidation states and bonding capacity for main group elements using their electron structure.
C4.8h / I can describe the shape and orientation of s and p orbitals.
C4.8i / I can explain why the electron location cannot be exactly determined at any given time.
C4.9A / I can identify elements with similar chemical and physical properties using the periodic table.
C4.9b / I can identify metals, non-metals, and metalloids using the periodic table.
C4.9c / I can predict general trends in atomic radius of the elements using the periodic table.
C4.9c / I can predict the general trend for first ionization energy of the elements using the periodic table.
C4.9c / I can predict the general trend for electronegativity of the elements using the periodic table.

Chapter 7 (Ionic Bonding), 8(Covalent Bonding and Intermolecular Forces) and 9 (Chemical Names and Formulas)

HSCE / Target/s:
I can statements. / Give an example that demonstrates your knowledge of the target or explain the target in your own words.
C3.2b / I can describe the relative strength of single, double, and triple covalent bonds between nitrogen atoms.
C4.2A / I can name simple binary compounds using their formulae.
C4.2B / I can write the formula of simple binary compounds when given the name.
C4.2c / I can name the compound when given the formula.
C4.2d / I can write the formula of ionic and molecular compounds when given the name.
C4.3c / I can compare the relative strengths of forces between molecules based on the melting point and boiling point of the substances.
C4.3e / I can predict whether the forces of attraction in a solid are primarily metallic, covalent, network covalent, or ionic based upon the elements’ location on the periodic table.
C4.3 h / I can explain properties of various solids such as malleability, conductivity, and melting point in terms of the solid’s structure and bonding.
C4.3i / I can explain why ionic solids have higher melting points than covalent solids. (For example, NaF has a melting point of 995°C while water has a melting point of 0° C.)
C4.4b / I can identify if a molecule is polar or nonpolar given a structural formula for the compound.
C5.5A / I can predict if the bonding between two atoms of different elements will be primarily ionic or covalent.
C5.5B / I can predict the formula for binary compounds of main group elements.
C5.5c / I can draw Lewis structures for simple compounds.
C5.5d / I can compare the relative melting point hardness for ionic, metallic, and covalent compounds.
C5.5d / I can compare the electrical and thermal conductivity for ionic, metallic, and covalent compounds.
C5.5d / I can compare the hardness for ionic, metallic, and covalent compounds.
C5.5e / I can relate the melting point of a substance to its structure.
C5.5e / I can relate the hardness of a substance to its structure.
C5.5e / I can relate the electrical and thermal conductivity of a substance to its structure.
C4.3c / I can compare the relative strengths of forces between molecules based on the melting point and boiling point of the substances.
C4.3d / I can compare the strength of the forces of attraction between molecules of different elements. (For example, at room temperature, chlorine is a gas and iodine is a solid.)
C4.3e / I can predict whether the forces of attraction in a solid are primarily metallic, covalent, network covalent, or ionic based upon the elements’ location on the periodic table.
C4.3f / I can identify the elements necessary for hydrogen bonding (N, O, F).
C4.3g / I can given the structural formula of a compound, indicate all the intermolecular forces present (dispersion, dipolar, hydrogen bonding).
C4.3h / I can explain properties of various solids such as malleability, conductivity, and melting point in terms of the solid’s structure and bonding.
C4.4a / I can explain why at room temperature different compounds can exist in different phases.
C5.4c / I can explain why both the melting point and boiling points for water are significantly higher than other small molecules of comparable mass (e.g., ammonia and methane).
C5.4e / I can compare the melting point of covalent compounds based on the strength of IMFs (intermolecular forces).