1-5 Measurement
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Accuracy refers to how close a measurement is to the accepted value, while precision refers to how close repeated measurements are to each other. Three students collected density data for sucrose and recorded their measurements over three trials. Student A's measurements were the least accurate but most precise, while Student C's measurements were the most accurate but least precise based on how close their average densities were to the accepted value of 1.59 g/cm3 and how close their individual trials were to each other.
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The document discusses acids and bases. It defines acids as substances that produce hydrogen ions (H+) in water and bases as substances that produce hydroxide ions (OH-). It lists examples of acids and bases and discusses their characteristics, including their effect on pH. It also discusses factors that affect reaction rates and methods for testing whether a substance is acidic or basic, such as pH indicators and the litmus test.
5-3 Balancing Moles
This document defines the mole as the standard unit used by chemists to count particles and explains how moles are used to balance chemical equations. It states that one mole is equal to 6.022 x 1023 particles of a substance and that different substances have different molar masses based on their atomic or molecular masses. It also describes how moles allow chemists to show the conservation of mass in chemical reactions by converting between mass and moles using molar mass.
5-1 Describing Reactions
The document discusses chemical reactions and balancing chemical equations. It explains that chemical reactions involve reactants combining to form products, with compounds changing forms. Mass is conserved in chemical reactions, with the total mass of reactants equaling the total mass of products. It also provides examples of how to count atoms in chemical formulas using subscripts and coefficients.
5-2 Balancing Reactions
This document discusses balancing chemical equations by manipulating coefficients to ensure conservation of mass. It provides examples of balancing a variety of chemical equations including reactions involving polyatomic ions, metals, nonmetals, hydrogen, and oxygen. The key steps are to count the number of atoms on each side of the equation and adjust coefficients until balanced.
4-4 Ionic & Covalent Bonding
Ionic bonds form when electrons are transferred between metals and nonmetals, resulting in oppositely charged ions. Covalent bonds form when nonmetals share electrons in order to achieve a stable electron configuration. Ionic compounds have high melting points and conduct electricity well when melted but not solid, while covalent compounds have low melting points and generally do not conduct electricity or dissolve in water well.
4-1: Ions & Ionic Bonding
1) Atoms form ions when they lose or gain electrons to achieve a stable electron configuration like the noble gases.
2) Metals form positive ions (cations) by losing electrons, while nonmetals form negative ions (anions) by gaining electrons.
3) Ionic bonds form when oppositely charged ions are attracted to each other, such as sodium (Na+) and chlorine (Cl-), resulting in an ionic compound.
3-6 Modern Periodic Table
The document discusses the periodic table and properties of elements. It describes how the elements are arranged by increasing atomic number in rows called periods and columns called families or groups. Properties repeat as you go across periods, with metals becoming less metallic and nonmetals becoming more reactive. There are three main classes of elements - metals, nonmetals, and metalloids between metals and nonmetals. Metals are shiny, malleable, conductive solids, while nonmetals are dull, brittle, non-conductive gases or solids with low melting points.
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