Chemistry Terms

123456789101112131415161718192021222324252627
Across
  1. 2. Subatomic particle with a 0 charge, mass of 1amo and located in the center of the atom. Different atoms of the same element can have different numbers of this particle although there are most common amounts for each element. This most common amount is found by subtracting the number of protons of the element from the mass number (the atomic mass rounded to the nearest whole number)
  2. 5. One atom of an element that has gained or lost electrons and now has a charge.
  3. 7. Found by subtracting the number of electrons from the number of protons or by considering the number of electrons gained or lost. This is negative if electrons are gained and positive if electrons are lost. For neutral atoms this value is 0. For ions this value is almost always +1, +2, +3, -1, -2 or -3.
  4. 8. This number is the number of protons plus the number of neutrons for one atom of an element. This number is not the same for all atoms of the same element because of changes in numbers of neutrons. The most common number for an element can be found by rounding the atomic mass to the nearest whole number.
  5. 10. A set of atoms covalently bonded together to form one distinct unit.
  6. 13. A way of representing the location of electrons. This can tell what energy levels are on, how many electrons are in each energy level and what orbitals are used. Electrons can be represented using superscripts or arrows. The shortened version of this notation uses noble gases to replace the initial energy levels.
  7. 14. In chemistry this is a number placed to the right and slightly above an element symbol or an energy level. This number is slightly smaller than the regular script. This number represents ion charge when placed after an element symbol and number of electrons when placed after an energy level.
  8. 15. The “rooms” in an energy level. Each one can contain 2 electrons with opposite spin (facing opposite directions). S energy levels contain 1 of these, p orbitals contain 3, ds contain 5 and fs contains 7.
  9. 17. The center of the atom where protons and neutrons are located.
  10. 20. The abbreviated form of an element name. Used in chemical formulas. Consists of 1 or 2 letters. The first letter is always capitalized. If there is a second letter it is always lowercase. Each element has its own unique set of letters.
  11. 21. Found on the left side of the periodic table, these elements are required in an ionic bond. These elements will give away electrons and form the positively charged ion. These are typically shiny and malleable and able to conduct electricity.
  12. 23. All elements want to have 8 valence electrons and will, give, take or share electrons to get to 8 valence electrons. (the one main exception is Hydrogen which only wants 2).
  13. 24. This can be ionic or covalently bonded but is a set of atoms connected together through their electron interactions
  14. 25. Same as the chemical or element symbol but must include a charge indicating a gain or lost of electrons from the neutral atomic form.
  15. 26. Elements in the last column of the periodic table. They do not react because their energy levels are all filled. All other elements try to be like them by gaining or losing elections. These can be used in electron configurations to indicate that the electron configuration of the 2 elements is the same with some additional electrons in the other element’s structure.
  16. 27. This is used to give the number and type of atoms found in a compound. This uses element symbols to give the elements and subscripts to indicate how many atoms of each element exist in that compound.
Down
  1. 1. In chemistry this is a number placed to the right and slightly below an element symbol in a chemical formula. This number indicates how many atoms of an element can be found in one unit of a compound. An example of this is the 2 in the formula H2O
  2. 3. Found on the right side of the periodic table of elements. These are the other half of an ionic compound but are the only type of elements needed to form covalent bonds. In an ionic compound these will take electrons and form the negative ion. In a covalent bond these will share electrons. The only one of these not found on the right side of the periodic table is hydrogen.
  3. 4. A set of ions bonded together to form a group of ions. This group must contain both positive and negatively charged ions.
  4. 6. this is the number of electrons involved in the bonding process. This is most often not equal to the total number of electrons. For ions this number is used to determine if electrons will be gained or lost. In covalent bonds, the number needed to reach 8 total is equal to the number of bonds that will form. These electrons can be represented in a Lewis Dot Diagram. This number can be found at the top of each column on the periodic table followed by the letter A. There is always a number associated with every element. Those values will always be between 1 and 8.
  5. 9. The average mass of 1 atom of an element. This number, rounded to the nearest whole number, can be used to calculate the most common number of neutrons for one atom of an element. This number can be found at the bottom of the box for an element on the periodic table.
  6. 11. The “floors” on which electrons live. These are commonly labeled s, p, d, or f and numbered 1-7. Each level, s, p, d, and f, contains different levels of orbitals.
  7. 12. Subatomic particle with a positive 1 charge, mass of 1amu and located in the center of the atom. It determines what element an atm is. The number of this particle is equal to the atomic number for the element.
  8. 16. The general space around the nucleus where the electrons are located in energy levels and orbitals.
  9. 18. One particle of an element made up of protons and neutrons in the nucleus and electrons in the electron cloud. These can be combined to form ionic compounds or molecules.
  10. 19. Subatomic particles with a negative 1 charge, no mass and located in energy levels around the center of the atom. The number of this particle in a neutral atom is equal to the number of protons. When an atom forms an ion this particle is either gained or lost to fill the outermost valence shell. The gaining, losing or sharing of this particle is what allows atoms to bond to form compounds.
  11. 22. This number comes from the number of protons an element has. It is also equal to the number of electrons in a neutral atom. This number can be found at the top of the box for an element on the periodic table