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Introductory Chemistry Flashcards > Basic chemistry > Flashcards

Basic chemistry Flashcards

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1
Q

what are the seven diatomic elements and what are their states at room temperature

A

(gas) oxygen
(gas) hydrogen
(gas) fluorine
(greenish gas) chlorine
(red liquid) bromine
(gas) nitrogen
(purple volotile solid) iodine (iodine can sublime directly into a gas)

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2
Q

what are covalent bonds (1 point)

A

a sharing of electrons, since they have same electronegativeily , hydrogen + hydrogen is a non-polar covalent bond

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3
Q

what are ionic bonds

A

they are assosicated with a tranfer of electrons, typically contain a metal and a non-metal

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4
Q

ploar covalent bond

A

electrons are shared unequally
if electronegativity different is considered to be equal to or more than 0.5 its polar, if its less its usually non-polar

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5
Q

what is a pure substance

A

has a constant composition, can be elements, compounds

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6
Q

what is a mixture

A

a combination of multiple pure substances, and can have variable composition

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7
Q

what is a homogenous mixture

A

mixture where the pure substances mix together (e.g. salt water), you don’t see the two disinguishable parts

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8
Q

what is a heterogenous mixture

A

mixture where the pure substances don’t mix together (e.g. oil and water, sand and water)

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9
Q

physical change vs chemical change

A

chemical identity changes in a chemical change,

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10
Q

phyiscla propoerties

A

boiling point
melting point
ductility
malleability
colour
viscosity
density
mass, weight, volume

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11
Q

chemical properties

A

flammability
corrosive
combustible
explosive
colour changing
pH

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12
Q

law of conservation of mass

A

matter cannot be created or destroyed in a chemical reaction.

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13
Q

law of definite proportions

A

the masses of each element in a given compound have constant composition.

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14
Q

law of multiple proportions

A

the ratio of the masses of the 2nd element for different compounds can be reduced to whole numbers.

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15
Q

when is an atom negative

A

more electrons and protons

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16
Q

when is an atom positive

A

more protons than electrons

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17
Q

what is an ion

A

a particle with an unequal number of protons and electrons

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18
Q

what are cations

A

ions with positive charges, more protons than electrons, metals typically form cations

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19
Q

what are anions

A

ions with negative charges, more electrons than protons non-metal typically form anions.

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20
Q

what is a molecule

A

a molecule is a particle with multiple atoms

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21
Q

how to find no. of electrons

A

is equal to atomic number minus the charge of the species.

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22
Q

how to find no. of protons

A

is equal to atomic number of element

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23
Q

how to find the no. of neutrons

A

difference between mass number an atomic number

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24
Q

top number on elements

A

atomic number

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25
Q

bottom number on element

A

atomic mass

26
Q

what is the atomic number of an element

A

atomic number of element is its identity, e.g. all isotopes of nitrogen will have 11 as atomic number, but atomic mass can change and will change for different isotopes

27
Q

how to calculate average atomic mass of element through isotopic percentages

A

mass of isotope 1st x percentage in decimal form + mass of 2nd isotope x percentage in decimal form ………

28
Q

what is an isotope

A

an isotope are composed of same element, different mass, both have same atomic number.

Isotopes are substances that are composed of the same element but consist of different mass numbers and number of neutrons. They share the same atomic number and therefore the same number of protons.

29
Q

how to calculate percentage abundance of each isotopes

A

avefrage atomic mass = mass of isotope x percent abundance

A = M x L

e.g. 79.9 = 78.918 (x) + 80.916 (1 - x)
79.9 = 78.918x + 80.916 - 80.916x
-1.016 = -1.998x
x = 0.509

30
Q

what is an ion

A

An ion is a particle with unequal numbers of electrons and protons. Atoms have equal numbers of protons and electrons and are therefore electrically neutral.

31
Q

is an atom an ion, is an ion an atom???

A

i dont know dickhead

32
Q

ionic bond

A

Ionic bonds exist between metals and nonmetals and are made up of ions with positive and negative charges. occurs between ions. a transfer of electrons

33
Q

covalent bond

A

Covalent bonds involve a sharing of electrons where as ionic bonds are created by a transfer of electrons.

34
Q

what is an ionic compound

A

contains ions and has charges, 99% has a metal and a non-metal, keep in mind that amonium is always ionic.

more electronegtive element always ends in -ide, e.g., trichloride, oxide, etc.

35
Q

molecular compounds

A

both non-metals

36
Q

explain the chemical suffixes -ate, and -ite

A

No2- , -ate, -ite, ate has one more oxygen than ite, if you see ate or ite, its a polyatomic ion that has oxygen.

37
Q

polyatomic atoms (((4444)))

A

ions composed of many atoms

38
Q

what if atom has more oxygen than ate

A

put per infront of it, e.g., perchlorate

39
Q

what if you have something with one less oxygen than ite

A

put hypo in front of it, e.g., hypochlorite

40
Q

what is a compound

A

a substance comprised of two different elements

41
Q

how do you name anion

A

suffix -ide

42
Q

hydroxide
cyanide
chromate

chemical formulas

A

OH-
CN-
CrO4*2-

43
Q

how to name FeCl2 and FeCl3
(i think this is for transition metals)

A

iron (II) chloride
iron (III) chloride

44
Q

find number of Cu2S

A

2cu + s = 0
2x + (-2) = 0
(2x)/2 = 2
x = 1

45
Q

ionic compound with transition metals,

A

dont need to use tetra, tri, mono etc. i think

46
Q

how to name ion with suffix ide

A

hydro prefix, the ic suffix, then acid

47
Q

how to name ion with suffix ate

A

ic + acid

48
Q

how to name ion with suffix ite

A

ous + acid

49
Q

how much is a mole

A

6.022 x 10*23

purpose of mole is to represent a quantity of atoms particles

50
Q
A

nitrogen 14 atomic mass, means 14 grams per mole

51
Q
A

calcium phospate

Ca+2PO43- = Ca3(PO4)2

52
Q

how many moles of carbon atoms are present in 30g of carbon

A

30g C / 1 x 1 mol C / 12g C = 2.5 mol C

53
Q

how many atoms are present in 5 moles of zinc

A

5 mol Zn / 1 x 6.022 x 10^23 / 1 mol Zn = 3.011 x 10^24 atoms Zn

53
Q
A
53
Q

how many grams are there in 3.5 mols of carbon atoms

A

3.5 mol C / 1 x 12g C / 1 mol C = 42 g C

53
Q

how many moles of copper are equilvalent to 8 x 10^24 copper atoms

A

8 x 10^24 Cu atoms / 1 x 1 mol Cu / 6.022 x 10^23 atoms Cu = 13.28 mol Cu

53
Q

how many molecules of CO2 can be found in 55.1g of CO2?

A

CO2 -> C + 2(0)
-> 12.01 +2(16)
12.01 + 32
44.01 grams per mole (g/mol)

55.1g CO2 / 1 x 1 mol CO2 / 44.01g CO2 x 6.022 x 10^23 CO2 / 1 mol CO2 = 7.54 x 10^23 molecules of CO2

54
Q

rules for writing chemical formulas

A

1.Each atom present is represented by its element symbol.
2. The number of each type of atom is indicated by a
subscript written to the right of the element symbol.
3. When only one atom of a given type is present, the
subscript 1 is not written.

55
Q

definition of isotope

A

Atoms of an element which have the
same atomic number, but different atomic masses. i.e.
they have a different number of neutrons

56
Q
A

Introductory Chemistry Flashcards (15 decks)

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