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Unit 9 Physics Test
| Term | Definition |
|---|---|
| Negative charged Ion | Anion |
| The mass of the protons plus the mass of the neutrons equals _______? | atomic mass |
| What do the letters on the periodic table symbolize | atomic name |
| Every atom is arranged on the periodic table by counting its number of PROTONS. this number is called ______? | atomic number |
| The horizontal rows on the Periodic table are called _______? (this row also tells us how many orbitals shells the atom has) | atomic period |
| an abbreviation of each atom is printed on the periodic table and is called the... | atomic symbol |
| The 2nd most recent model of an atom was discovered by and named after what man? This is the model we use to draw atoms on. | Bohr Model |
| What are positively charged ions are called? | Cation |
| When atoms are bonded by sharing of electrons the bond is named...? | Covalent Bond |
| the rings or zones where the atom's electrons are stored are called? | Electron Shells |
| The soft, silvery-white, solid, metallic elements, with 1 electron in their outer shell, that are super reactive are known as what group? It will always form a cation. | Alkali Metals |
| The group or family that is a silvery metallic, reactive, solid, and has 2 electrons in its outer valence shell is called? It will always form a cation. | Alkali Earth Metals |
| What group has 3 electrons in its outer shell and is composed of a metals and a metalloid? It will always form a cation. | Boron Family |
| What group loves to make covalent bonds, is flexible at bonding and has 4 electrons in their outer shell? | Carbon Family |
| What group needs 3 electrons to form an octet and has 5 electrons in the outer shells and is a mix of metals, nonmetals and metalloids | Nitrogen Family |
| what group has 6 electrons in the outer shell and is a combination of metals and metalloids? | Oxygen Family |
| what group is highly reactive and creates salts and has 7 electrons in its outer shell plus requires one electron to fill the octet rule, and has a very high/strong electron affinity. | Halogens Family |
| What group has a full octet and does not combine with other atoms? | Noble Gases |
| a bond created by two atoms where one atom has a low electron affinity and one atom has a high electron affinity. The one with a high affinity will steal the electrons from the lower one to complete its octet. | Ionic Bond |
| How do you know how many electrons are in the "outer bonding shell" of any atom? | by the Family number (skipping the transition metals) |
| when an atom looses a neutron but still is the same atomic name it is called.... Example: Carbon 12 and Carbon 14 | Isotope |
| The outer most shell of all atoms is called...? hint:this is also the reason that the atom will bond due to the number of electrons in this outer most ring. | Valence Electrons |
| What is Ionization Energy? | The closer the element is to Hydrogen on the periodic table the more energy it has, it uses the Octet Rule (I SAID NO! DON'T TAKE MY ELECTRONS! IF YOU DO I WILL TURN INTO AN ION!) |
| What is Atomic Radius | The closer you are to Fr (Francium) the more shells you have (aka the fatter you are) and the more magnetism you have, the tighter you are. |
| What is Electromagnetically | Octet Rule. Arm Wrestling. There are 8 groups on the Periodic Table, each with 1-8 electrons. The more electrons you have, the more energy you have. |
| Rank the following elements by increasing atomic radius: Carbon, Aluminum, Oxygen, Potassium | Oxygen, Carbon, Aluminum, Potassium |
| Rank the following elements by increasing electronegativity: sulfur, oxygen, neon, aluminum | Neon, Aluminum, Sulfur, Oxygen |
| Why does fluorine have a higher ionization energy than iodine? | The closer you are to helium (the element holding onto it's electrons) the more energy you have |
| Why do elements in the same family generally have similar properties? | Same number of electrons |
| Indicate whether the following properties increase or decrease from left to right across the table. Atomic Radius (excluding noble gases) First ionization energy Electronegativity | Decrease Increase Increase |
| What trend in atomic radius occurs down a group on the periodic table? What causes this trend? | Gets another shell |
| What trend in ionization energy occurs across a period on the periodic table> What causes this trend? | Gets more and more electrons |
| Which is the largest atomic radius? AI or B | AI |
| Which is the largest atomic radius? Na or AI | Na |
| Which is the largest atomic radius? S or O | S |
| Which is the largest atomic radius? O or F | O |
| Which is the largest atomic radius? Br or Cl | Br |
| Which is the largest atomic radius? Mg or Ca | Ca |
| Which has the greater ionization energy? Li or Be | Be |
| Which has the greater ionization energy? Ca or Ba | Ca |
| Which has the greater ionization energy? Na or K | Na |
| Which has the greater ionization energy? P or Ar | Ar |
| Which has the greater ionization energy? Cl or Si | Cl |
| Which has the greater ionization energy? Li or K | Li |
| Define electronegativity | You gain electrons. The more electrons you have, the stronger you are |
| Which has the greater electronegativity? Ca or Ga | Ga |
| Which has the greater electronegativity? Br or As | Br |
| Which has the greater electronegativity? Li or O | O |
| Which has the greater electronegativity? Ba or Sr | Sr |
| Which has the greater electronegativity? Cl or S | Cl |
| Which has the greater electronegativity? O or S | O |
| Which statement best describes Group 2 elements from top to bottom? | The # of principal energy levels remains the same, and the # of valence electrons increases |
| What is the total # of valence electrons in an atom of boron in the ground state? | 3 |
| What is the total number of valence electrons in an atom of xenon, Xe? | 8 |
| The elements calcium and strontium have similar chemical properties because they both have the same... | # of valence electrons |
| Which element in Period 5 of the Periodic Table is a transition element? | Ag |
| Which of the following atoms has the largest atomic radius? | K |
| Which noble gas has the highest first ionization energy? | Helium |
| Which sequence of elements is arranged in order of decreasing atomic radii? AI, Si, P Li, Na, K Ba, Ra, Sr N, C, B | AI, Si, P |
| Which list of elements from Group 2 on the Periodic Table is arranged in order of increasing atomic radius? Be, Mg, Ca Ca, Mg, Be Ba, Ra, Sr Sr, Ra, Ba | Be, Mg, Ca |
| As each successive element in Group 15 of the Periodic Table is considered in order of increasing atomic number, the atomic radius? | Increases |
| The strength of an atom;s attraction for the electrons in a chemical bond is the atom's... | Electronegativity |
| Which properties are most common in nonmetals? | High ionization energy and high electronegativity |
| Which Group 17 element has the least attraction for electrons | I |
| Which element in Group 16 has the greatest tendency to gain electrons? | O |
| The group 17 element with the highest electronegativity is... | Fluorine |
| Which element in group 16 has the greatest tendency to gain electrons? Te, Se, S, or O | O |
| The group 17 element with the highest electronegativity is | Fluorine |
| As the elements of Group 1 on the Periodic Table are considered in order of increasing atomic radius, the ionization energy of each successive element generally | Decreases |
| The amount of energy required to remove the outermost electron from a gaseous atom in the ground state is known as | First ionization energy |
| Which element is a member of the halogen family? K, B, I, or S | I |
| Which of the following Group 2 elements has the lowest first ionization? Be, Mg, Ca, or Ba? | Ba |
| As the elements of Group 1 of the Periodic Table are considered in order from top to bottom, the ionization energy of each successive element decreases. This decrease is due to | Increasing radius and increasing shielding effect |
| Which sequence correctly places the elements in order of increasing ionization energy? H-Li-Na-K, I-Br-Cl-F, O-S-Se-Te, H-Be-AI-Ga | I-Br-Cl-F |
| Compared to the atomic radius of a sodium atom the atomic radius of a magnesium atom is smaller. The smaller radius is primarily a result of the magnesium atom having... | a larger nuclear charge |
| Which of these elements has the LEAST attraction for electrons in a chemical bond? oxygen, fluorine, nitrogen, chlorine | nitrogen |
| The ability of carbon to attract electrons is... | less than that of nitrogen and oxygen |
| As the elements Li to F in Period 2 of the Periodic Table are considered in succession, how do the relative electronegativity and the covalent radius of each successive element compare? | The relative electronegativity increases, and the atomic radius decreases |
| What would a line on a graph look like when showing the relationship between electronegativity and atomic number for elements of period 3 | positive linear |
| ELECTRONEGATIVITY (who will win) Mg + Cl | Cl |
| ELECTRONEGATIVITY (who will win) N + N | Neither they will share |
| ELECTRONEGATIVITY (who will win) K + Br | Br |
| ELECTRONEGATIVITY (who will win) Ai + P | Neither they will share |
| CATION OR ANION OR NO CHARGE Mo | Cation |
| CATION OR ANION OR NO CHARGE Br | Anion |
| CATION OR ANION OR NO CHARGE Mg | Cation |
| CATION OR ANION OR NO CHARGE Ar | No Charge |
| Who is the least reactive family | 8 |
| What Family is the alkaline earth metals | 2 |
| What family in named the halogens | 7 |
| what family is the noble gas family | 8 |
| what family is the alkali metal family | 1 |
| what family would have the least ionization energy | 1 |
| What family has the largest atomic radius. | 1 |
Created by:
26addison.agler