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IB Chemistry > matter, chemical trends, chemical bonding, and chemical reactions > Flashcards

matter, chemical trends, chemical bonding, and chemical reactions Flashcards

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1
Q

what is a group?

A
  • a column in the periodic table
  • members have similar physcial/chemical properties
  • they all have the same number of valence electrons
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2
Q

what is a period?

A

-a horizontal rowon the periodic table
-it corresponds to the number of energy levels they
have
-example: period 2 will have 2 has 2 energy levels

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3
Q

`what are blocks?

A
  • the periodic table is split up into 4 groups (s,p,d,f)

- these corresponds to the energy sublevels

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4
Q

what is the periodic law?

A

-when the elememts are arranged to increased atomic
number, elements with similar properties occur at
regular intervals

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5
Q

what are properties of metals?

A
  • shiny
  • malleable
  • conductor
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6
Q

what are properties of non-metals?

A
  • dull
  • brittle
  • insulator
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7
Q

alkali metals

A

-first group
-very reactive in water/air
-shiny, slivery, soft, malleable, good conductors,
soluable in water
-one electron in outer shell

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8
Q

alkaline earth metals

A
  • second group
  • not as reactive in water/air
  • shiny, silvery, soft, malleable, good conductors, soluable in water
  • two electrons in the outer shell
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9
Q

metalloids

A
  • on the staircase bewteen metals and non-metals
  • share some properties of metals/non-metals
  • example: silicon is shiny/somewhat conductive (metal) but its also brittle (non-metal)
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10
Q

halogens

A
  • second last group on thr periodic table
  • very reactive
  • solids, liquids, and gases
  • seven electrons in its outer shell
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11
Q

noble gases

A
  • last group in the periodic table
  • not reactive at all
  • all gases
  • full valence shell
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12
Q

transition metals

A
  • found in the D block

- found in the centre

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13
Q

lanthanides

A
  • these metals react similar to group two
  • found in F block
  • the sections of metals undeneath the table
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14
Q

actinides

A
  • they are the radioactive metals

- these metals are found in F block

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15
Q

why are alkali metals and halogens the most reactive?

A

-alkali metals only have one valence electron and want
to get rid of it
-halogens have an almost a full valence shell and they
want to get one more electron

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16
Q

why are nobles gasses the most stable?

A
  • because they have a full valence shell

- they dont want to gain or lose electrons

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17
Q

valence shell/electrons

A

-valence shell is the outer ring of the atom
-the valence electrons are only the electrons in the
outer most shell

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18
Q

element

A
  • made up of one type of atom

- cant be broken down into smaller forms

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19
Q

compounds

A

-made of two or more elements in a fixed ratio
-compounds have unique properties from the
elements that they are made up of

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20
Q

homogeneous mixture

A

-also called solutions
-the particles blend together in one phase and dont
separate upon setting
-solutions include a solute dissolved in a solvent
-example: air is made up of many different gases but
you cant see the different gases

21
Q

heterogeneous mixture

A
  • components are not uniformly mixed

- separates into two or more layers when settled

22
Q

what are the types of reactions?

A
  • synthesis
  • decomposition
  • combustion
  • single displacement
  • double displacment
23
Q

synthesis

A

-an element or small compound combines with one or
more elements/compounds to form a new substance
-a+b=ab

24
Q

decompostion

A

-a compound breaks down into elements/smaller
compounds
-ab=a+b

25
Q

combustion

A

-reaction of an element or compound with oxygen
-note any compound with carbon, hydrogen, or oxygen
makes CO2+H2O for products if theres is sufficient O2 avalible
-if not enough O2 is available incomplete combustion CO and C are made
-sulphur+oxygen=sulphur dioxide

26
Q

single displacement

A

-one element within a compound is replaced by
another element
-a+bc=b+ac

27
Q

double displacement

A
  • cations are traded between two ionic compounds

- ab+cd=cb+ad

28
Q

whats is an atom?

A
  • an atom is the smallest particle that retains the
    properties of an atom
    -atoms are very tiny and mostly empty space
29
Q

what is a sub-atomic particle?

A
  • protons
  • neutrons
  • electrons
30
Q

what is the charge, mass and location of a proton?

A
  • relative charge is +1
  • relative mass is 1
  • location is the nucleus
31
Q

what is the charge, mass and location of a neutron?

A
  • relative charge is 0
  • relative mass is 1
  • location is the nucleus
32
Q

what is the charge, mass and location of an electron?

A
  • relative charge is -1
  • relative mass is 1/2000
  • location is oribitingthe nucleus
33
Q

how many protons are in an element?

A

-the same amount as the atomic number

34
Q

how many electrons are in an element?

A

-the same amount as the atomic number
-if there is an extra charge at the top of the number you
add that number to the atomic number and the anser
is the number of electrons

35
Q

how many neutrons are in an element?

A

-the mass number subtract the atomic number

36
Q

isotope

A

-atoms of the same element that have different

numbers of neutrons

37
Q

isotope abundance

A
  • the frequency each isotope appear in an element

- it is always expressed as a % decimal

38
Q

average atomic mass

A

-the average of all masses of all isotopes taking into
their account their isotopic abundance
-how to calculate: 1. multiple mass of each isotope by
its abundance 2. find the sum of these values

39
Q

what is the equation for average atomic mass?

A

-7(0.9258)+6(0.0742)
-lithium-7 occurs 92.58% of the time and lithium-6
occurs 7.42% of the time
-the number infront of the brackets are the type of
element and the number inside the brackets are the
percent they occur but in decimal form

40
Q

how do you find the isotopic abundance?

A
  • average mass=%B-10(10)+%B-11(11)
  • find the average mass of the elemant on the periodic table and let the first part of the equation equal x and the second part equal 1-x
  • 10.81=x(10)+(1-x)(11)
  • 10.81=10x+11-11x
  • 10.81=11-x
  • x=0.19
  • so B-10 has the abundance of 19% and B-11 has the adundance of 81%
41
Q

name the trends of the periodic table

A
  • atomic radius
  • ionic radius
  • first ionization energy
  • electronegativity (en)
  • matallic behaviour
  • electron affinity
42
Q

atomic radius

A

-the distance measured from the centre of the necleus
to the outer most electron
-increases as you move down a group-why: as you
move down a group there are more energy level
between the necles and valance shell
-decreases as you move across a period-why: as you
move across the number of protons in the necleus
increases this increases its postive pull the necleus
has on the electrons orbiting it pulling the necleus.

43
Q

ionic radius

A

-metals lose electrons to become cations, non-metals
gain electrons to become anions
-the ions beloware isoelectronic-they have different
atomic numbers but the same numberof electrons as
eachon the (Ne)
-trend-ionic radius increases the number of the protons
decreases

44
Q

First ionization energy

A

-the amount of energy needed to remove an electron
from the atom
-decreases as you move down a group-why: the atomic
size is larger and the valence electrons are farther
from the nucleus so the pull on electrons from the
nucleus’s lower
-increases as you move across a period-why: the
attraction between the nucleus and the electron is
increasing due to the increasing number of protons in
the nucleus this causes it to be more difficult for
electrons to be pulled off

45
Q

Electronegativity (en)

A
  • the ability to attract electrons in a bond
  • increases across periods and decreases down groups
  • the en difference between 2 atoms helps us decide the type of bond that will form
46
Q

Metallic behaviour

A
  • metals are malleable/good conductors if heat/electricity

- metallic behaviour decreases across abs period and increases down a group

47
Q

Electronic affinity

A
  • the amount of energy released when an electron is attached to a neutral atom
  • it can also be looked at as the likelihood of an atom to become an anion
  • increases across periods/decreases down groups
48
Q

Lewis structure

A
  • diagram only showing the valence electrons of an element

- the electrons are placed every 90 degrees until they have to repeat again

IB Chemistry (1 decks)

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