Exam 1 Flashcards

Question

P

Answer 1

phosphorus

Answer 2

molybdenum

Answer 3

kilogram (kg)

Answer 4

kelvin (K)

Answer 5

second (s or sec)

Answer 6

mole (mol)

Answer 7

μ 1x10^-6

Answer 8

p 1x10^-12

Answer 9

f 1x10^-15

Answer 10

- non-zeros are always significant - zeroes between non-zeroes are significant - zeroes before the first non-zero are not significant - zeroes at the end of a decimal are significant

Answer 11

result has the same number of sig figs as the number in the question with the fewest amount

Answer 12

result has the same number of places after the decimal point as the number with the fewest number after the decimal

Answer 13

- g/mL (liquids) - g/cm^3 (solids)

Answer 14

- all matter is made of atoms - atoms of a given element are identical in mass and properties - atoms can't be subdivided, created, or destroyed - atoms combine in simple, whole-number ratios to form compounds - law of conservation of mass, law of multiple proportions, law of constant composition

Answer 15

- mass can't be created or destroyed, only changed in arrangement - the total mass of substances remains constant during a reaction

Answer 16

if elements A and B react to form more than one compound, the different masses of B that combine with a fixed mass of A can be expressed as a ratio of small whole numbers

Answer 17

the composition of a given compound does not change – any sample will have the same mass percentages of its component elements

Answer 18

the number on top of the element symbol

Answer 19

number below the element symbol

Answer 20

protons= atomic number (number on top of the element)

Answer 21

electrons are the same as protons in an atom because they have a neutral charge (number on top of the element)

Answer 22

mass number - atomic number (number on the bottom - number on the top)

Answer 23

convert abundance to a decimal/ fraction and multiply it by the mass of each isotope, then add all the numbers together

Answer 24

right side

Answer 25

along the line separating them

Answer 26

representative/ main group elements

Answer 27

transition metals

Answer 28

groups or families

Answer 29

column/ group/ family

Answer 30

alkali metals

Answer 31

alkaline earth metals

Answer 32

noble gasses

Answer 33

elements 57-71

Answer 34

elements 89-103

Answer 35

positively charged ions (lose electrons)

Answer 36

negatively charged ions (gain electrons)

Answer 37

Positive Ions (Cations) NH4+ ammonium Hg22+ mercury(I) Negative Ions (Anions) 1- NO3– nitrate NO2– nitrite HCO3– bicarbonate ClO4– perchlorate ClO3– chlorate ClO2– chlorite ClO– hypochlorite BrO4– perbromate BrO3– bromate BrO2– bromite BrO– hypobromite IO4– periodate IO3– iodate IO2– iodite IO– hypoiodite CH3COO– acetate CN– cyanide SCN– thiocyanate OH– hydroxide MnO4– permanganate O2– superoxide 2- CrO42– chromate Cr2O72– dichromate SO42– sulfate SO32– sulfite S2O32– thiosulfate CO32– carbonate O22– peroxide C2O42– oxalate 3- AsO43– arsenate PO43– phosphate PO33– phosphite

Answer 38

HCl = hydrochloric acid HBr = hydrobromic acid HI = hydroiodic acid HNO3 = nitric acid H2SO4 = sulfuric acid HClO4 = perchloric acid HClO3 = chloric acid

Answer 39

CH3COOH = acetic acid H3PO4 = phosphoric acid H2S = hydrosulfuric acid HCN = hydrocyanic acid HCOOH = formic acid HF = hydrofluoric acid HNO2 = nitrous acid

Answer 40

NaOH = sodium hydroxide LiOH = lithium hydroxide KOH = potassium hydroxide RbOH = rubidium hydroxide CsOH = cesium hydroxide Ca(OH)2 = calcium hydroxide Ba(OH)2 = barium hydroxide

Answer 41

NH3 = ammonia C5H5N = pyridine CH3NH2 = methylamine

Answer 42

1. Pure elements (including those that exist as diatomics) are assigned a zero for their ON. 2. Monatomic ions have an ON equal to their common charge. * Metals always have a positive charge. * Group 1A metals have an ON = +1 * Group 2A metals have an ON = +2 * Other metals often have a charge equal to their group number on the Periodic Table (NOTE: This is not true for elements like the transition metals that have more than one oxidation number.). 3. The ON of a non-metal depends on what other elements it is bonded to, but can be assigned in the following order: * Fluorine (F) has an ON of -1, ALWAYS! * Hydrogen (H) has an ON of +1 (Note: H has an ON of -1 when bound to a metal). * Oxygen has an ON of -2 (Note: O has an ON of +2 when bound to F, O has an ON of -1 in peroxide and -1/2 in superoxides). * Halogens (Group 7A) have an ON of -1. * The most electronegative atom is assigned a charge first (equal to that of its common charge) if all the atoms in a compound are non-metals. 4. The sum of all the ONs in a compound/ion must add up to the overall charge of the compound/ion. For neutral compounds, this charge is zero

Answer 43

Write the name of the cation (positively-charged ion, often a metal) first. * If the cation is a polyatomic ion, write the name of the polyatomic cation as is. * If the cation is a transition metal or a metal that has more than one oxidation number, put the charge in Roman numerals after the metal in parentheses. o Ag, Zn, Cd are all transition metals but only have ONE oxidation number so a Roman numeral is not needed. 2. Write the name of the anion (negatively-charged ion, often a nonmetal) second. * If the anion is an element, write the name of the element, with the –ide ending (drop the last syllable and add –ide), after the cation. * If the anion is a polyatomic ion, write the name of the polyatomic anion as is after the cation.

Answer 44

Prefix-first atom (**The prefix mono- is NOT included on the first atom.) * Prefixes: mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, octa-, nona-, deca- * If there is only one of the first atom in the molecular compound, the mono- prefix is dropped. 2. Prefix-second atom root-ide * Prefixes: mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, octa-, nona-, deca- * Drop “o” or “a” from the prefix if the element begins with a vowel

Exam 1 Flashcards

(134 cards)