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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
What's ionization energy?
the energy needed to completely remove an electron from a gaseous atom or ion
26
What's a peroxide?
An oxygen ion that will only bond with **group 1** elements ex: Fr2O2 ~ francium peroxide
27
How do you name acids that contain oxygen?
HFO4 = perfluor**ate** (change to ic acid) --> perfluoric acid HFO3 = fluor**ate** (change to ic acid) --> fluoric acid HFO2 = fluor**ite** (change to ous acid) --> fluorous acid HFO = hypofluor**ite** (change to ous acid) --> hypofluorous acid
28
What's electronegativity
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
How do you name a binary molecular compound?
* 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
What are the charges of protons, neutrons, and electrons?
Protons = positive Neutrons = neutral Electrons = negative
31
What does the prefix **thio** mean?
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
What are binary compounds
compounds that consist of atoms of 2 elements (mostly a metal and a non-metal)
33
What's the london dispersion force?
an attractive force acting between all molecules, including non-polar molecules ~ the weakest intermolecular force
34
What's the first ionization energy?
the energy required to remove the first valence electron from a neutral atom
35
What's Charles Gas Law
as temperature increases, volume increases as temperature decreases, volume decreases V1/T1 = V2/T2
36
What happens to atomic radius as you move across a period from left to right?
it decreases
37
How do you name acids with a monoatomic ion?
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
What's hydrogen bonding?
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
What's the dipole-dipole force?
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
How do you name acids with polyatomic ions?
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
How do you convert Celsius to kelvin? How do you convert kelvin to celsius?
Celsius to kelvin = °C + 273.15 kelvin to celsius = kelvin - 273.15
42
What's a binary molecular compound?
compounds that are made up of 2 nonmetals ex: CO2 ~ carbon dioxide
43
What happens to ionization energy moving down a group on the periodic table?
ionization energy decreases
44
what does avagadros gas law state?
a gas law stating that equal volumes of all ideal gasses at the same temperature and pressure contain the same number of molecules
45
what does combined gas law state?
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
what does gay lussacs law state
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
what does charles law state
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
what does boyles gas law state?
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
what is ideal gas law?
a gas law that describes the relationship between pressure, volume, temperature, and amount (in moles) of an ideal gas law. PV=nRT
50
What is Dalton's Law of Partial Pressures?
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
What is a covalent bond?
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
whats a polar covalent bond?
a covalent bond in which electron distribution is unequal ~ a covalent bond formed between two atoms with significantly different electronegativities
53
what do polar bonds have?
a positive pole and a negative pole ~ ex. dipole bonds
54
How do you know if a bond is ionic, polar covalent, etc.?
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
What are coordinate covalent bonds?
a covalent bond in which both electrons come from the same atom
56
What are van der waals forces?
weak intermolecular attractions * including LONDON DISPERSION forces & DIPOLE-DIPOLE forces
57
What is a polar molecule?
a molecule that is slightly positively charged at one end and slightly negatively charged at the other because of electronegativity differences
58
whats a chemical reaction
a chemical change where one or more substances are destroyed and one or more new substances are created
59
whats a synthesis reaction
2 or more reactants combine to form a complex substance/product
60
what are the different types of synthesis?
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
whats a decomposition reaction
the compound (product) breaks down into its elements or substances (the reactants)
62
what are the different types of decompoistion reactions
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
whats a combustion reaction
reaction that involves oxygen gas as a reactant and a hydrocarbon (CxHy)
64
whats complete combustion and what does it produce?
complete combustion is where there is abundant/excess oxygen gas ~ only produces water (H20) and carbon dioxide (CO2)
65
whats incomplete combustion and what does it produce?
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
in what order do you have to balance a combustion reaction
balance carbon first, balance hydrogen second, balance oxygen third
67
Whats the kinetic molecular theory of gases?
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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