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Chemistry (Grade 11) > Final Exam > Flashcards

Final Exam Flashcards

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1
Q

What’s atomic radius?

A

distance from the nucleus to the valence shell of a neutral atom
~measured in picometers (pm)

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2
Q

what is effective nuclear charge?
what happens when it goes across a period, and down a group?

A

how much the electrons are attracted to the nucleus of an atom.
–> it increases across a period, decreases down a group.

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3
Q

what is an isotope?

A

atoms with the same number of protons but different number of neutrons

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4
Q

what are the families on the periodic table

A

group 1 - alkali metals
group 2 - alkaline earth metals
Groups 3-12 - transition metals
group 17 - halogens
group 18 - noble gases

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5
Q

What’s the family of 4 for polyatomic ions?

A

CIO4 - = perchlorate
CIO3 - = chlorate
CIO2 - = chlorite
CIO - = hypochlorite

~ look at notebook for more details and practice

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6
Q

how are elements in the same family similar

A

they have the same number of valence electrons

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7
Q

What’s the Gay - Lussac’s Gas Law?

A

as pressure increases, temperature increases

as pressure decreases, temperature decreases

P1/T1 = P2/T2

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8
Q

As you move left to right on the periodic table, what happens?

A
  • atomic radius decreases
  • ionization energy increases
  • electronegativity increases
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9
Q

What is the ideal gas law? What is the R value?

A

PV = nRT

R is the universal gas constant (8.314 KPaL mol^-1k^-1)

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10
Q

What are the guidelines to use ideal gas law

A
  • convert temp. to kelvin
  • convert mass to mols
  • convert volume to litres
  • convert pressure to KPa
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11
Q

What’s electron affinity?

A

the energy absorbed or released when an electron is added to a neutral atom

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12
Q

what happens to electron affinity as you go up a group

A

it increases

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13
Q

what happens to electron affinity as you go across a period

A

it increases

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14
Q

How do you name acids that do not contain oxygen?

A
  • hydro (root) ic acid

ex: hydrogen fluoride (HF)
~ hydrofluoric acid

ex: hydrogen cyanide (HCN)
~ hydrocyanic acid

ex: hydrogen sulfide (H2S)
~ hydrosulfuric acid

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15
Q

What’s the second ionization energy?

A

the energy required to remove a second electron from the univalent ion to form the divalent ion

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16
Q

What happens to atomic radius as you move down a given group?

A

it increases

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17
Q

How do you name a binary ionic compound?

A
  • name the metal ion first, then the non-metal
  • if the metal is a TRANSITION METAL, it can have more than one charge (roman numerals in brackets after the name of the metal to indicate charge)
  • the suffix of the non-metal is changed to ide (ex. oxygen –> oxide)

example: Fe2O3
~ Iron (III) oxide

example: Ca (NO3)2
~ calcium nitrate

example: AuCl3
~ Gold (III) chloride

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18
Q

What is Avogadro’s Gas Law?

A

states that equal volumes of all ideal gases at the same temperature & pressure contain the same # of molecules

n1/v1= n2/v2

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19
Q

What happens to ionization energy as you move left to right across a period on the periodic table?

A

ionization energy increases

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20
Q

What intermolecular force is present in ionic bonds?

A

electrostatic force

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21
Q

Whats the absolute zero?

A

the lowest theoretical temperature; -273.15°C

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22
Q

What is Boyle’s Gas Law?

A

as pressure increases, volume decreases

as pressure decreases, volume increases

P1V1=P2V2

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23
Q

As you move down a given group, what happens?

A
  • atomic radius increases
  • ionization energy decreases
  • electronegativity decreases
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24
Q

What’s the Combined Gas Law?

A

law of combining volumes

p1v1/T1 = p2v2/T2

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25
Q

What’s ionization energy?

A

the energy needed to completely remove an electron from a gaseous atom or ion

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26
Q

What’s a peroxide?

A

An oxygen ion that will only bond with group 1 elements

ex: Fr2O2
~ francium peroxide

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27
Q

How do you name acids that contain oxygen?

A

HFO4 = perfluorate (change to ic acid) –> perfluoric acid

HFO3 = fluorate (change to ic acid) –> fluoric acid

HFO2 = fluorite (change to ous acid) –> fluorous acid

HFO = hypofluorite (change to ous acid) –> hypofluorous acid

28
Q

What’s electronegativity

A

a measure of the attraction of an atom for the electrons in a chemical bond
~ an indicator of the relative ability of an atom to attract shared electrons

29
Q

How do you name a binary molecular compound?

A
  • name the element with the lower group # first
  • exception: if oxygen is combined with a halogen (group 7) then the halogen is named first
  • name of the 1st element is unchanged
  • add ide to the suffix of the second element
  • if there are two or more atoms of the first atom, indicate the # of atoms
  • always add a prefix to the second element to show the # of atoms

ex: N2O4
~ dinitrogen tetroxide

ex: SF6
~ Sulfur hexafluoride

ex: PCl5
~ phosphorus pentachloride

30
Q

What are the charges of protons, neutrons, and electrons?

A

Protons = positive
Neutrons = neutral
Electrons = negative

31
Q

What does the prefix thio mean?

A

it means that an oxygen in the compound has been replaced by a sulfur atom

EX: SO4 ^2- is Sulphate
~ S2O3 ^2- = thiosulphate
~ S2O2 ^2- = thiosulphite

32
Q

What are binary compounds

A

compounds that consist of atoms of 2 elements
(mostly a metal and a non-metal)

33
Q

What’s the london dispersion force?

A

an attractive force acting between all molecules, including non-polar molecules

~ the weakest intermolecular force

34
Q

What’s the first ionization energy?

A

the energy required to remove the first valence electron from a neutral atom

35
Q

What’s Charles Gas Law

A

as temperature increases, volume increases

as temperature decreases, volume decreases

V1/T1 = V2/T2

36
Q

What happens to atomic radius as you move across a period from left to right?

A

it decreases

37
Q

How do you name acids with a monoatomic ion?

A

ide –> hydro (root) ic acid

As the monoatomic ion ends with ide, put hydro before the root of the monoatomic ion and add the ic acid at the end.

example: HCl
~ hydrochloric acid

example: H2S
~ hydrosulfuric acid

example: HCN
~ CN- is cyanide
~ name: hydrocyanic acid

38
Q

What’s hydrogen bonding?

A

attraction of hydrogen atoms bonded to nitrogen, oxygen, and fluorine in adjacent molecules
~ a relatively strong dipole-dipole force that can only occur between O-H, N-H, and F-H bonds

39
Q

What’s the dipole-dipole force?

A

force of attraction between POLAR molecules
~ the attractive forces between the positive end of one polar molecule and the negative end of another molecule

40
Q

How do you name acids with polyatomic ions?

A

ate –> ic acid
ite –> ous acid

If the polyatomic ion ends with ate, change it to ic acid. If the polyatomic ion ends with ite, change it to ous acid.

example: HNO3
~ NO3- is nitrate
~ therefore the name is nitric acid

example: H2SO3
~ SO3 ^2- is sulfite
~ therefore the name is sulfurous acid

41
Q

How do you convert Celsius to kelvin? How do you convert kelvin to celsius?

A

Celsius to kelvin = °C + 273.15

kelvin to celsius = kelvin - 273.15

42
Q

What’s a binary molecular compound?

A

compounds that are made up of 2 nonmetals

ex: CO2
~ carbon dioxide

43
Q

What happens to ionization energy moving down a group on the periodic table?

A

ionization energy decreases

44
Q

what does avagadros gas law state?

A

a gas law stating that equal volumes of all ideal gasses at the same temperature and pressure contain the same number of molecules

45
Q

what does combined gas law state?

A

a gas law stating that the pressure and volume of a given amount of gas are inversely proportional to each other and are directly proportional to the kelvin temparture of the gas.

46
Q

what does gay lussacs law state

A

a gas law stating that the pressure of a fixed amount of gas at a constant volume is directly proportional to its kelvin temperature.

47
Q

what does charles law state

A

a gas law stating that the volume of a fixed amount of gas at a constant pressure is directly proportional to the kelvin temperature of the gas.

48
Q

what does boyles gas law state?

A

a gas law stating that the volume of a fixed amount of gas at a constant temperature is inversely porotional to the applied (external) pressure on the gas

49
Q

what is ideal gas law?

A

a gas law that describes the relationship between pressure, volume, temperature, and amount (in moles) of an ideal gas law.
PV=nRT

50
Q

What is Dalton’s Law of Partial Pressures?

A

a gas law which states that the total pressure of a mixture of gases is the sum of the individual pressures of each gas

51
Q

What is a covalent bond?

A

attraction between atoms from the sharing of electrons
~ a chemical bond formed when electrons are shared between atoms

involves electrostatic attractions between the positively charged nuclei and the negatively charged electrons
if the electronegativity of 1 of the 2 atoms that are bonded together is greater than the electronegativity of the other atom, the electrons will be attracted more strongly to the first atom

52
Q

whats a polar covalent bond?

A

a covalent bond in which electron distribution is unequal
~ a covalent bond formed between two atoms with significantly different electronegativities

53
Q

what do polar bonds have?

A

a positive pole and a negative pole
~ ex. dipole bonds

54
Q

How do you know if a bond is ionic, polar covalent, etc.?

A

you know from the ΔEN

ΔEN > 1.7 = mostly ionic
ΔEN is between 0.4 - 1.7 = polar covalent
ΔEN < 0.4 = slightly polar covalent
ΔEN = 0 –> non polar covalent

55
Q

What are coordinate covalent bonds?

A

a covalent bond in which both electrons come from the same atom

56
Q

What are van der waals forces?

A

weak intermolecular attractions
* including LONDON DISPERSION forces & DIPOLE-DIPOLE forces

57
Q

What is a polar molecule?

A

a molecule that is slightly positively charged at one end and slightly negatively charged at the other because of electronegativity differences

58
Q

whats a chemical reaction

A

a chemical change where one or more substances are destroyed and one or more new substances are created

59
Q

whats a synthesis reaction

A

2 or more reactants combine to form a complex substance/product

60
Q

what are the different types of synthesis?

A

1) two elements form a binary compound (ex. Na + Cl –> NaCl)
2) two non-metals form a molecular compound (ex. C + O2 –> CO2)
3) non-metal oxide and water form an oxyacid (CO2 + H2O –> H2CO3)
4) metal oxide and water form a base (Na2O + H2O –> NaOH)

61
Q

whats a decomposition reaction

A

the compound (product) breaks down into its elements or substances (the reactants)

62
Q

what are the different types of decompoistion reactions

A

1) binary compounds break down into their elements (NaCl –> Na + Cl2)
2) metal nitrate breaks down (–>) into the metal nitrite and oxygen gas (ex. NaN03 –> NaNO2 + O2)
3) metal carbonate breaks down into the metal oxide and carbon dioxide (ex CaCO3 –> CaO + CO2)
4) metal hydroxide breaks down into the metal oxide and water (ex. NAOH –> Na2O + H20)

63
Q

whats a combustion reaction

A

reaction that involves oxygen gas as a reactant and a hydrocarbon (CxHy)

64
Q

whats complete combustion and what does it produce?

A

complete combustion is where there is abundant/excess oxygen gas
~ only produces water (H20) and carbon dioxide (CO2)

65
Q

whats incomplete combustion and what does it produce?

A

incomplete combustion is where there is limited oxygen gas
~ produces water (H20), carbon dioxide (CO2), carbon monoxide (CO) and carbon (C)
* this carbon can be soot

66
Q

in what order do you have to balance a combustion reaction

A

balance carbon first, balance hydrogen second, balance oxygen third

67
Q

Whats the kinetic molecular theory of gases?

A

Kinetic molecular theory states that gas particles are in constant motion and exhibit perfectly elastic collisions

Chemistry (Grade 11) (8 decks)

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