Target Set 2 Quiz

2.3 I can write element symbols in isotopic notation.

A q X Z X=Element Symbol A=Mass Number (Protons + Neutrons) Z=Atomic Number (Number of Protons) q=Charge (Number of electrons, if neutral 0, if negative charge, +e and if positive, -e)

2.1 I can describe the atom, its parts (protons, neutrons, and electrons) and location of these parts and their characteristics.

Atom: The smallest particle of an element that retains its identity in a chemical reaction. Proton: A positively charged subatomic particle found in the nucleus of an atom. Mass is 1.67x10^-24 or 1 amu. Neutron: A subatomic particle with no charge and a mass of 1.68x10^-24 or 1 amu; found in the nucleus of an atom. Electrons: A negatively charged subatomic particle with a mass of 9.1x10^-27 or 1/1833 amu that orbits in the electron cloud around the nucleus.

2.11 I can use the periodic table to calculate molar mass for an element.

Molar mass: The mass of 1 mole of the element or compound. This is given on the periodic table of elements. The units are in g/m or grams/mole. Ex) 1 H 1.0079 The 1.0079 of hydrogen is the average molar mass of all of the isotopes.

2.4 I can figure out the atomic number, mass number, and number of electrons in a neutral atom or ion of an element.

Neutral Ex) 23 (0) Na 11 Na has 11 protons, it is neutral so it has no charge so there are the same number of electrons as protons (11), and the mass number minus the protons is 23-11=12, so there are 12 neutrons. Ion Ex) 35 -1 Cl 17 Cl has 17 protons, 35-17=18 so there are 18 protons, and there is a charge of -1, so there is one EXTRA electron, so there are 18 electrons.

2.12 I can preform the following calculations (using dimensional analysis and considering sig figs) with the mole. •Grams to moles •Moles to grams •Moles to atoms (particles) •Atoms (particles) to moles •Grams to moles to atoms (particles) •Atoms (particles) to moles to grams

REMEMBER: There are 6.02x10^23 particles or atoms in a mole. Grams to moles: Grams/1 x 1 mole/Molar mass Moles to grams: Moles/1 x Molar mass/1mole Moles to atoms (particles): Moles/1 x 6.02*10^23/1 mole Atoms (particles) to moles: Atoms/1 x 1 mole/6.02&10^23 Grams to moles to atoms: Grams/1 x 1 mole/molar mass x 6.02*10^23/mole Atoms to moles to grams atoms/1 x 1 mole/6.02*10^23 x molar mass/1 mole

2.10 I can describe the mole as a counting unit and state "how much" a mole is- expressed in scientific notation (Avogadro's number).

The mole is a counting unit equal to 6.02x10^23.

2.2 I can recognize scientists' models of the atom from past to present day and place them chronologically along a timeline.

Use chart for pictures Democritus 400 BC Sea Shell Model- Believed objects are made of atoms. John Dalton 1808 Billiard Ball Model- Everything is made of atoms, they are indivisible and indestructible. Discovered the electron and performed a cathode-ray experiment. J.J. Thomson 1897 Plum Pudding Model- Passed light rays through atoms which made him believe there is something negatively charged and something positively charged. Marie Curie 1898 Radioactivity- First to discover radioactivity by the use of radium and polonium. Ernest Rutherford 1911 Gold Foil- Shot alpha positive rays, some bounced back and some went through, discovered the nucleus. Neils Bohr 1913 Rings- Explained electrons are energy shells that orbit the nucleus in a defined pattern. Each electron had a fixed energy level. Robert Millikan 1923 Electrons- He discovered that the electrons which orbit the nucleus are negatively charged. He discovered the mass of the electron too. Werner Heisenberg 1925 Charge Cloud Model- Atom is very spacious, shows it is mostly big space but close to the nucleus is the biggest cloud which contained negative electrons. Erwin Schrodinger 1926 Quantum- Discovered electrons are traveling in orbitals. James Chadwick 1932 Neutrons- The nucleus contains neutrons and protons, while the electrons orbit the nucleus in layers. Lise Meitner 1938 Nuclear Fission- Hahn, Meitner, and Strassmann became the first to recognize that the uranium atom, when bombarded by neutrons, actually split.

2.6 I can describe what happens when electrons absorb/release different amounts of energy and a. Relate the change in energy to the color of light and the electromagnetic spectrum. b. Distinguish between ground state and excited state.

When an electron is in a state of lowest possible energy, it is in a ground state. If it absorbs energy, it jumps from one level of energy to a higher one. This means it is in an excited state. Electrons don't like to be excited, because it is unstable. To avoid this, the electron falls back down to its original state. When this electron falls back to the original state, it releases energy in the form of electromagnetic radiation/light. The greater the distance the electron falls, the more energy is released. In terms of visible light, the order of lowest to highest is ROYGBIV.

2.5 I can a. Predict the particles and electromagnetic waves produced by different types of radioactive decay. b. Write equations for nuclear decays. c. Describe the characteristics of alpha, beta, and gamma radiation and their ability to penetrate materials (penetrability). d. Calculate half-life

a. α=alpha, same as He. Has 4/2. β=beta, same as e if negative. If positive, it is called a positron. Has 0/+-1 γ=gamma, has 0/0 b.When writing equations, pay attention to isotope, that is the top number. The bottom number is the number of protons, as found on the periodic table. Next, draw arrow and write the given symbol (alpha, beta, gamma). Find the element with the correct number of protons to balance out both sides, and write the correct isotope number to balance as well. *If fission, it will go from a small amount to a large amount and will have neutron 1/0. If fusion, it will go from large amount to small amount and fuse. Sometimes, there may also be p for proton which is 1/1. c. Alpha- External is not harmful, bad if ingested or inhaled, blocked by paper or skin. Beta-Often acompanied by gamma radiation, beta minus is produced b/c neutron splits into p+ and e-, blocked by plastic. In a positron, the positron collides with electron and results in gamma radiation, proton becomes a neutron. Gamma- dangerous, can be blocked by lead vest, used in medical therapies. d. Not learned yet.