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pre ap chemistry 1 > district exam :( > Flashcards

district exam :( Flashcards

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1
Q

ion

A

an atom that has lost or gained one or more electrons

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2
Q

cation

A

ion with a positive charge, metals, loses electrons

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3
Q

anion

A

an ion with a negative charge, gains electrons, nonmetals

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4
Q

octet rule

A

atoms lose, gain, or share valence electrons to have eight valence electrons in order to be stable

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5
Q

what charge does a zinc ion always have

A

2+

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6
Q

what charge does silver ion always have

A

1+

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7
Q

IUPAC

A

international union of pure and applied chemistry

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8
Q

what does IUPAC do

A

responsible for setting the standards for atomic mass values, measurements, nomenclature

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9
Q

monatomic ion

A

a single atom that gains or loses electrons

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10
Q

how do you name monatomic ions that are cations

A

-write the parent name then write ion

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11
Q

how do you name monatomic ions that are anions

A

write the parent name, add -ide then write ion

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12
Q

note for naming monatomic anions

A

you usually add the ide after the first syllable

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13
Q

when do you use the stock system

A

transition elements and group 14 because they form more than one cation

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14
Q

how do you use the stock system

A

write the name of the element, followed by a roman numeral to indicate charge

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15
Q

when do you NOT use stock system

A

for zinc or silver because they form one ion

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16
Q

chemical formula

A

abbreviation for substance or molecule with element symbols and substances in a definite ratio

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17
Q

binary ionic compounds

A

a compound that includes one cation and one anion (a metal and a non metal)

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18
Q

writing binary ionic compounds

A

write the symbol and charges for the metal and nonmetal. criss cross the charges, drop the sign and write each number as a subscript (except 1)

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19
Q

exception for writing binary ionic compounds

A

the charges will cancel if its a positive and negative of the same number. ex: Fe2+ S2- becomes FeS

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20
Q

naming binary ionic compounds

A

name the cation, name the anion and change the end to -ide, use stock system for transition metals

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21
Q

polyatomic ion

A

a charged group of two or more bonded atoms that are bonded together by a covalent bond

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22
Q

polyatomic compund

A

a compound that includes a cation and a polyatomic ion

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23
Q

what do parentheses do in a polyatomic compound

A

separate an ion and its subscript

24
Q

writing polyatomic compounds

A

write the symbol for the cation and the polyatomic ion, criss cross the charges, drop the sign, write each number as a subscript. use parentheses

25
Q

naming polyatomic compounds

A

name the cation and polyatomic ion, use the stock system for transition metals and group 14

26
Q

covalent compound

A

a compound that consists of two nonmetals

no charges because electrons are shared

27
Q

ionic compounds are

A

neutral

28
Q

naming covalent compounds

A

use a prefix that indicated number of atoms present

do not use mono with the first element

if the second element has “ao” or “oo” drop the firt vowel

second word ends in ide

29
Q

acid

A

a compound in which one or more H+ ions bond to a negative ion

30
Q

naming acids without oxygen

A
  • break the acid into H+ and its negative ion
  • for the negative ion, drop the -ide and place the stem between hydro and ic
  • add the word acid
31
Q

acids without oxygen numonic

A

my ride has hydrolics

32
Q

naming acids with oxygen (ate)

A
  • break the acid into H+ and its polyatomic ion
  • for the negative polyatomic ion, drop the -ate and add “ic”
  • add the word acid
33
Q

naming acids with oxyegn (ate) nummonic

A

I ate something icky

34
Q

naming acids with oxygen (-ite)

A
  • breal the acid into its H+ and its polyatomic ion
  • for the negative polyatomic ion, drop teh -ite and add ous
  • add the word acid
35
Q

naming acids with oxyegn (-ite) nummonic

A

sprite is delicious

36
Q

H3PO4

A

phosphoric acid

37
Q

H3PO3

A

phosphorous acid

38
Q

H2SO4

A

sulfuric acid

39
Q

H2SO3

A

sulfurous acid

40
Q

chemical bond

A

forces that hold atoms together

41
Q

bonding pair

A

an electron pair that is shared

42
Q

lone paire

A

an electron pair that is not shared

43
Q

7

A

hepta

44
Q

4

A

tetra

45
Q

note for acids

A

the number of hydrogens is the charge of the anion

46
Q

VSEPR

A

Valence Shell Electron Pair Repulsion Theory

47
Q

what does VSEPR do

A

model that predicts the geometry of a molecule considering electrons want to be far away from each other

48
Q

single bond

A

one pair of shared electrons

49
Q

double bond

A

two pairs of shared electrons

50
Q

triple bond

A

three pairs of shared electrons

51
Q

drawing VSEPR strucutres

A
  • find number of electron pairs
  • LEAST electronegative atom is the central atom
  • draw the bonding pairs as lines to connect
  • place pairs around outisde atoms
  • place left over pairs around the central atom
52
Q

electronegativity

A

increases from left to right

increases up

53
Q

how to find number of electron pairs

A

count all VE
for polyatomic ions, add the charge for a negative ion, subtract the charge if the ion is positive
-divide total VE by 2

54
Q

the shape it will be

A

trigonal pyramidal

55
Q

areas of electron density/ electron domains/ dense electron zone

A

areas where there are pairs of electrons on the central aom

56
Q

areas of electron density/electron domains/dense electron zones hat form bonds

A

here there are bonding pairs on the central atom l,

pre ap chemistry 1 (12 decks)

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