Chemistry Unit 1: Atomic Structure & Periodic Table

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Questions and Answers

What are periods? What do they represent with regard to the anatomy of an atom?

Periods are the horizontal rows on the periodic table. They represent the number of electron shells in an atom.

What are groups/families? What information is determined by this number?

Groups/families are the vertical columns on the periodic table. They represent the number of electrons in the outermost shell, which is also known as valence electrons.

Identify where the following are found on the periodic table: (Select all that apply)

  • Noble gasses (correct)
  • Metals (correct)
  • Alkaline Earth metals (correct)
  • Lanthanide and Actinide series (correct)
  • Nonmetals (correct)
  • Halogens (correct)
  • Metalloids (correct)
  • Transition metals (correct)
  • Alkali metals (correct)

What is “normal conditions” or STP?

<p>Standard temperature and pressure, typically defined as 0°C or 273.15K and 1 atmosphere of pressure.</p> Signup and view all the answers

Which two elements are liquid at normal conditions? Which elements are gasses? Solids?

<p>Mercury and Bromine (B), Helium and Neon (D)</p> Signup and view all the answers

What are the 7 diatomic elements?

<p>Hydrogen (H2), Nitrogen (N2), Oxygen (O2), Fluorine (F2), Chlorine (Cl2), Bromine (Br2), and Iodine (I2)</p> Signup and view all the answers

Match the following programming languages with their primary usage:

<p>Python = General-purpose programming JavaScript = Client-side scripting for web applications SQL = Database queries CSS = Styling web pages</p> Signup and view all the answers

What are the three subatomic particles, their charges, masses and respective locations in the atom?

<p>Protons (positive charge, located in the nucleus), neutrons (no charge, located in the nucleus), and electrons (negative charge, orbiting the nucleus)</p> Signup and view all the answers

What are valence electrons?

<p>The electrons in the outermost shell of an atom, which are involved in chemical bonding.</p> Signup and view all the answers

Determine from the periodic table the number of valence electrons for a given element.

<p>The number of valence electrons for an element can be determined by its group number in the periodic table.</p> Signup and view all the answers

What is the significance of Rutherford's experiment in relation to atomic structure?

<p>Rutherford's experiment revealed that atoms have a dense nucleus, leading to the discovery of protons and transformation of the atomic model.</p> Signup and view all the answers

Explain the difference between a cation and an anion.

<p>A cation is a positively charged ion formed by the loss of electrons, while an anion is a negatively charged ion formed by the gain of electrons.</p> Signup and view all the answers

How do you determine the mass of a particular isotope?

<p>The mass of an isotope is determined by adding the number of protons and neutrons in its nucleus.</p> Signup and view all the answers

What is meant by the term 'isotope'?

<p>An isotope refers to variants of a chemical element that have the same number of protons but different numbers of neutrons.</p> Signup and view all the answers

What are valence electrons and why are they important?

<p>Valence electrons are the electrons found in the outermost shell of an atom and are crucial for chemical bonding.</p> Signup and view all the answers

Flashcards

Atom

The smallest unit of an element that retains the chemical properties of that element.

Proton

A positively charged particle found in the nucleus of an atom.

Neutron

A neutral particle found in the nucleus of an atom.

Electron

A negatively charged particle that orbits the nucleus of an atom.

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Atomic Number

The number of protons in the nucleus of an atom.

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Mass Number

The sum of protons and neutrons in the nucleus of an atom.

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Isotopes

Atoms of the same element that have the same number of protons but different numbers of neutrons.

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Periodic Table

A chart that organizes all the known chemical elements by atomic number, electron configuration, and recurring chemical properties.

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Period

A horizontal row of elements in the periodic table.

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Group

A vertical column of elements in the periodic table.

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What is STP?

Standard Temperature and Pressure (STP) is a set of standard conditions used for scientific measurements, typically defined as 0 degrees Celsius (273.15 Kelvin) and 1 atmosphere of pressure.

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What are valence electrons?

Valence electrons are the electrons in the outermost shell of an atom. They are the ones involved in chemical bonding.

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How do you determine the most common oxidation state of an element?

The most common oxidation state for an atom is determined by its position on the periodic table, specifically its group number. For example, elements in Group 1A typically have a +1 oxidation state, while elements in Group 7A typically have a -1 oxidation state.

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What did Rutherford's experiment reveal?

Rutherford's experiment involved firing alpha particles at a thin gold foil. Some particles passed straight through, while others were deflected or even bounced back. This showed that atoms are mostly empty space with a dense, positively charged nucleus in the center.

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What is an isotope?

An isotope is an atom of the same element that has the same number of protons (atomic number) but a different number of neutrons. This results in a different mass number.

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Study Notes

Unit 1: Atomic Structure and the Periodic Table

  • Know the element symbols and names for elements 1-30, 33-36, 46-47, 50, 51, 53-56, 74, 78-80, 82, 86-87, 92.
  • Know the symbols and names of all elements and polyatomic ions on the provided sheet.
  • Understand periods and groups/families, their relation to the anatomy of an atom, and how to identify both.
  • Know the locations of metals, nonmetals, metalloids, transition metals, alkali metals, alkaline earth metals, halogens, noble gases, lanthanides, and actinides on the periodic table.
  • Define "normal conditions" or STP.
  • Identify elements that are liquid and gaseous at normal conditions.
  • Know the 7 diatomic elements.
  • Know the three subatomic particles (protons, neutrons, electrons), their charges, masses, and locations within an atom.
  • Define valence electrons.
  • Determine the number of valence electrons for an element based on its position on the periodic table.
  • Determine the most common oxidation state for an element based on its periodic table position.
  • Explain Rutherford's experiment and its key findings.
  • Define atomic number.
  • Define isotope and how to determine its mass.
  • Define cation and how it forms.
  • Define anion and how it forms.
  • Know the difference between mass number and average atomic mass.
  • Explain how to calculate average atomic mass.
  • Provide two ways to write a nuclide for a given isotope.
  • Calculate the number of protons, neutrons, electrons, and mass for ions and isotopes.
  • Define electrical and chemical stability, and which is more crucial.
  • Identify elements that are generally chemically stable and their location on the periodic table.
  • Know the "magic number" for chemical stability for most elements.
  • Identify exceptions to the octet rule and how they still satisfy chemical stability.

Unit 2: Electrons of the Atom

  • Understand how properties of elements arise from their atomic structures.
  • Elements in the same group exhibit similar properties.
  • Elements in the same period have a similar number of electron shells.
  • Reactivity is determined by the atomic structure and electron arrangement.
  • Define octet rule and exceptions related to Helium, Hydrogen, Lithium, Beryllium, and Boron.
  • Define ground state and excited state of an electron.
  • The number of sublevels on each energy level.
  • Define orbital.
  • The number of orbitals in each sublevel.
  • The maximum number of electrons that can occupy an orbital.
  • Draw electron configurations and orbital diagrams for given atoms.
  • Draw electron configurations for cations and anions.
  • Write noble gas configurations for given atoms.
  • Draw orbital diagrams for elements.
  • Understand Aufbau, Hund's rule, and Pauli exclusion principle and where they apply to orbital diagrams.
  • Explain the four quantum numbers and their ranges.
  • Identify an element given its quantum number address
  • Hierarchy of electron configurations for relative stability in elements.
  • Elements and configurations for maximum stability.
  • Explain what a full outer energy level and a full sublevel mean.
  • Maximum number of electrons that can fill each sublevel.

Unit 3: Thermochemistry

  • Conversion factors between calories, kilocalories, joules, and kilojoules.
  • Use dimensional analysis for unit conversions in heat energy.
  • Determine the number of significant figures in calculations.
  • Define q (heat), associated units and the SI unit (joules).
  • Define m (mass), and the accepted unit (grams).
  • Define ΔT (change in temperature), the calculation (final temperature – initial temperature) and unit (degrees Celsius, Kelvin).
  • Define C (specific heat capacity) and its derived units (J/g°C or J/gK).
  • Understand how heat changes from the point of view of the system versus the surroundings.
  • Explain the difference between heat capacity and specific heat capacity.
  • Define temperature and its SI unit (Kelvin).
  • Calculate kinetic energy and understand that the component that most affects kinetic energy is mass.
  • Determine the SI unit for heat (joules), and temperature (Kelvin).
  • Know the magic number for converting temperatures to Kelvin (multiply Celsius by 9/5, then add 273.15).
  • Explain any color changes in beakers when dry ice is added to a "witch's brew" solution (if this was part of the original text, otherwise, skip this).
  • Understanding how straight lines represent/display data (constant rates of change).
  • Explain any extra practice instructions, such as reviewing previous homework or worksheets, etc.

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