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Introduction to Chemistry Exam 1 Study Guide

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Termini in questo insieme (28)

  • What is the definition of Chemistry?

    Chemistry is the study of matter, its properties, how and why substances combine or separate, and how substances interact with energy.

  • How do you count significant figures in a number?

    Significant figures include all non-zero digits, zeros between significant digits, and trailing zeros in a decimal number.

  • What is dimensional analysis used for?

    Dimensional analysis is used to convert between units by multiplying by conversion factors, such as inches to feet or seconds to minutes.

  • How do you convert units using prefixes like milli, micro, kilo, and mega?

    Use the prefix values to multiply or divide: milli = 10-3, micro = 10-6, kilo = 103, mega = 106.

  • What is the density equation?

    Density is calculated as \(\rho = \frac{m}{V}\), where m is mass and V is volume.

  • What are the main steps of the scientific method?

    Observation, hypothesis, experimentation, scientific laws, and theories.

  • What are uncertain digits in measurements?

    Uncertain digits are the last digit in a measurement that is estimated and not exact.

  • Name some common units of measurement in chemistry.

    Units include meters (m), liters (L), grams (g), seconds (s), and moles (mol).

  • What is the difference between elements, molecules, and compounds?

    An element is a pure substance of one type of atom; a molecule is two or more atoms bonded; a compound is a molecule with different elements.

  • What are the properties of the different states of matter?

    Solids have fixed shape and volume, liquids have fixed volume but no fixed shape, gases have neither fixed shape nor volume.

  • How is matter classified using mixture, pure substance, element, compound, heterogeneous, and homogeneous?

    Pure substances have uniform composition; mixtures contain two or more substances; heterogeneous mixtures have visibly different parts; homogeneous mixtures are uniform throughout.

  • How do you identify physical and chemical changes?

    Physical changes alter appearance without changing composition; chemical changes produce new substances.

  • What are endothermic and exothermic reactions?

    Endothermic reactions absorb heat; exothermic reactions release heat.

  • How do you calculate heat using water's specific heat?

    Use \(q = m \times c \times \Delta T\), where q is heat, m is mass, c is specific heat, and ΔT is temperature change.

  • What are some common separation techniques in chemistry?

    Techniques include filtration, distillation, chromatography, and centrifugation.

  • What does the Law of Conservation of Mass state?

    Mass is neither created nor destroyed in a chemical reaction; total mass remains constant.

  • What are the different forms of energy relevant to chemistry?

    Forms include kinetic, potential, thermal, chemical, and nuclear energy.

  • What are the properties of the different subatomic particles?

    Protons are positive, neutrons are neutral, electrons are negative; protons and neutrons are in the nucleus, electrons orbit around it.

  • How do you identify elements from the main groups of the periodic table?

    Main groups include alkali metals, alkaline earth metals, halogens, and noble gases, each with characteristic properties.

  • What are the common charges of atoms in main groups?

    Group 1: +1, Group 2: +2, Group 17: -1, Group 18: 0 (noble gases).

  • What are isotopes?

    Isotopes are atoms of the same element with different numbers of neutrons.

  • How do you calculate using the natural abundance equation?

    Calculate average atomic mass by summing (isotope mass × fractional abundance) for all isotopes.

  • How do you count protons, electrons, and neutrons in elements and ions?

    Protons = atomic number; electrons = protons ± charge; neutrons = mass number - protons.

  • How do you calculate the ratio of elements in a compound?

    Use moles of each element to find the simplest whole number ratio.

  • What is the difference between empirical and molecular formulas?

    Empirical formula shows simplest ratio of atoms; molecular formula shows actual number of atoms.

  • What are diatomic molecules?

    Diatomic molecules consist of two atoms, such as H2, N2, O2, F2, Cl2, Br2, and I2.

  • How do you write names and formulas for ionic compounds, binary molecular compounds, and acids?

    Ionic compounds combine cations and anions; binary molecular compounds use prefixes for number of atoms; acids often start with 'hydro-' and end with '-ic acid'.

  • How do you name ionic, molecular compounds, and acids?

    Name cation first, then anion; use prefixes for molecular compounds; acids named based on anion ending (e.g., -ate to -ic acid).