Grade 11 Chemistry Exam

Front 1

What is the pattern of metallic characters of the elements on the periodic table?

Back 1

increases from top to bottom in a group and from right to left in a period

Front 2

The greater the electronegativity of an atom the greater the tendency of the element to?

Back 2

gain electrons

Front 3

What is the most electronegative element?

Back 3

fluorine

Front 4

What is ionization energy?

Back 4

the energy required to remove an electron from a neutral atom in its gaseous phase.

Front 5

Which elements have higher ionization energies?

Back 5

Elements on the right side, because their valence shell is nearly filled

Front 6

Why do elements on the left side of the periodic table have lower ionization energies?

Back 6

because of their willingness to lose electrons and become cations

Front 7

What is the pattern of ionization energy of an element on the periodic table?

Back 7

Increases from left to right, increases down to up

Front 8

What is the pattern of electronegativity of an element on the periodic table?

Back 8

Increases from left to right, increases down to up

Front 9

What is electron affinity?

Back 9

the ability of an atom to accept an electron

Front 10

The more negative the electron affinity value, the higher an atom's.....

Back 10

affinity (attraction) for electrons

Front 11

What is the pattern of electron affinity of the elements on the periodic table?

Back 11

Electron affinity increases from left to right within a period,decreases from top to bottom within a group

Front 12

Why does electron affinity increase from left to right in a period?

Back 12

caused by the decrease in atomic radius

Front 13

Why does electron affinity decreases from top to bottom within a group?

Back 13

caused by the increase in atomic radius

Front 14

Why does ionization energy increase from left to right in a period?

Back 14

valence shell stability

Front 15

Why does ionization energy increase from bottom to top in a group?

Back 15

electron shielding

Front 16

Why do the noble gases possess high ionization energies?

Back 16

because of their full valence shells

Front 17

What is the atomic radius?

Back 17

The atomic radius is one-half the distance between the nuclei of two atoms

Front 18

What is the pattern of atomic radius of the elements on the periodic table?

Back 18

-decreases from left to right within a period

-increases from top to bottom within a group

Front 19

Why does atomic radius increase from right to left in a period?

Back 19

-caused by the increase in the number of protons and electrons across a period. One proton has a greater effect than one electron; thus, electrons are pulled towards the nucleus, resulting in a smaller radius.

Front 20

Why does atomic radius increase from bottom to top?

Back 20

-caused by electron shielding

Front 21

What is a covalent bond?

Back 21

-non metal + non metal

-formed when atoms share electrons to become stable

Front 22

What are the conditions under which a covalent bond forms?

Back 22

-electronegativity of elements must be high

-ionization of elements must be high

Front 23

What is an ionic bond?

Back 23

- metal+non metal

-bond formed with elements of opposite charges

Front 24

What are the conditions necessary for an ionic bond to form?

Back 24

-must be metal + non metal

Front 25

how can you tell if a bond has ionic character?

Back 25

the bigger the difference between the electronegativity of two atoms, the more likely it is to be ionic

Front 26

how can you tell if a bond has covalent character?

Back 26

If the electronegativity is the same between elements, then the bond is likely covalent

Front 27

What are the characteristics of covalent substances?

Back 27

-low melting point

-low boiling point

-slow rate of reaction

-do not conduct electricity

Front 28

What are the characteristics of ionic substances?

Back 28

-high melting point

-high boiling point

-dissolve easily in water

-do not conduct electricity when solid

-when melted, conduct electricity

Front 29

What is the activity series?

Back 29

A series of metals, in order of reactivity from highest to lowest

Front 30

What is the activity series used for?

Back 30

The activity series is a useful guide for predicting the products of metal displacement reactions

Front 31

what destroys polarity of molecules?

Back 31

symmetry

Front 32

what are the propertries of a base?

Back 32

-bitter

-no smell (except for ammonium)

-turn red litmus paper blue

-feel slippery to skin

-pH greater than 7

Front 33

what are the properties of an acid?

Back 33

-sour

-turn blue litmus paper red

-sticky feel

-pH less than 7

Front 34

what occurs during a chemical change?

Back 34

-new substance is formed

-changes colour

-precipitate forms

-difficult to reverse

Front 35

what occurs during a physical change?

Back 35

-size

-shape

-state of matter

-can be reversed

Front 36

what are the 5 types of reactions?

Back 36

-synthesis

-decomposition

-single displacement

-double displacement

-combustion

Front 37

the elements with the lowest ionization energies are the....

Back 37

alkali metals

Front 38

metallic oxides dissolved in water form...

Back 38

a base

Front 39

what type of reaction is the combustion of metal?

Back 39

synthesis reaction

Front 40

when sodium is burned in the air, what is the formula of the oxide?

Back 40

Na2O

Front 41

isotopes of an element differ in...

Back 41

mass number

Front 42

what is the atomic number of an element based on?

Back 42

number of protons in the atom

Front 43

True or false: a solution is a heterogeneous mixture

Back 43

true

Front 44

true or false: all portions of a mixture that have the same properties belong to the same phase

Back 44

true

Front 45

true or false: pure samples of any compound obey the law of definite proportions

Back 45

true

Front 46

true or false: the components of a solution can be separated through physical means

Back 46

false

Front 47

true or false: adding a tiny crystal to a super saturated solution usually starts crystalization

Back 47

true

Front 48

true or false: the solubility of all gases increases with increasing temperature

Back 48

false

Front 49

true or false: an unsaturated solution can dissolve more solute

Back 49

true

Front 50

true or false: the solubility of most solids increases with increasing temperature

Back 50

true

Front 51

true or false: cooling an unsaturated solution may cause it to become saturated

Back 51

true

Front 52

what is an arrhenius base?

Back 52

a substance that increases the concentration of hydroxide (OH-) ions in the solution when dissolved in an aqueous solution

Front 53

in an aqueous solution, what does salt exist in the form of?

Back 53

ions

Front 54

what decreases as gas is cooled at a constant volume?

Back 54

-kinetic energy of molecules

-pressure of the gas

Front 55

real gases' behaviours deviate from ideal gases' behaviour under what conditions?

Back 55

-very low temperatures

-very high pressures

Front 56

what does Avogadro's law state?

Back 56

a mole of any gas occupies 22.41 Liters at 1 atmosphere pressure and 0 degrees celsius

Front 57

Explain the opposing trends of ionization energies and atomic radii in the alkali group of the Periodic table

Back 57

The bigger the element, the easier it is to take an electron from its outer shell, due to shielding and distance