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?

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

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

Mercury and Bromine Signup and view all the answers

What are the 7 diatomic elements?

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

Match the following programming languages with their primary usage:

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

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

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

What are valence electrons?

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

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

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

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

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

Explain the difference between a cation and an anion.

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. Signup and view all the answers

How do you determine the mass of a particular isotope?

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

What is meant by the term 'isotope'?

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

What are valence electrons and why are they important?

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

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).

Unit 4: Periodic Trends

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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Description

Test your knowledge on atomic structure and the periodic table with this quiz. Covering elements 1-30, their symbols, and the properties of metals, nonmetals, and metalloids, this quiz will challenge your understanding of chemistry fundamentals. Get ready to identify groups, periods, and key concepts like valence electrons and oxidation states!