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Chemistry 11U - 2023 > Unit 1 Test Review > Flashcards

Unit 1 Test Review Flashcards

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1
Q

What is the periodic law associated with the organization of the periodic table?

A

-elements are arranged in order of increasing atomic number
-elements with similar physical and chemical properties occur at regular intervals using this order
*DIMITRI MENDELEEV

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2
Q

What are the three basic types of elements found on the periodic table?

A

Metals
Non-metals
Metalloids

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3
Q

Describe metal elements

A

state: solid except mercury
physical properties:
-hard, lustrous
-good conductors of heat and electrical current
-malleable and ductile

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4
Q

Describe non-metals

A

state: many gas, some solid, one liquid (bromine)
physical properties:
-non-lustrous
-poor conductor of electrical current and heat
-brittle and non-ductile

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5
Q

Describe metalloids

A

state: all
physical properties:
-good conductors of electrical current
-poor conductors of heat
-brittle

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6
Q

What is a period?

A

-a horizontal row on the periodic table
-period number indicates the energy level (shell) of the valence electrons

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7
Q

What is a group/family?

A

-vertical column on the periodic table
-group number indicates valence electron number

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8
Q

What are the standard states of all elements?

A

solid
liquid
gas

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9
Q

What are synthetic elements?

A

-elements that are outlined with a black border and white fill
-they are synthetically produced via nuclear fusion in nuclear reactors or particle accelerators

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10
Q

In what category are most elements involved in creating living tissue found?

A

other non-metals

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11
Q

Why does each period end with a noble gas

A

each noble gas has a stable amount of electrons

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12
Q

What is an atom?

A

the building block of matter
make up everything but energy
-the smallest particle of an element that still retains the identity and properties of the element

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13
Q

What are atoms made out of?

A

3 subatomic particles:
-neutrons
-protons
-electrons

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14
Q

Explain the electron arrangement in atoms

A

-according to Borh’s diagrams, electrons exist in orbits around the nucleus
-each orbit has a specific level of energy associated with it
-the further away an electron is from the nucleus, the more energy the electron possesses
-electrons in the outermost orbit are called valence electrons, and they help form chemical bonds between atoms
-when electrons are removed, they gain a positive charge and these are called cations
-when electrons get added, these are negative and called anions

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15
Q

What does it mean for an atom to be isoelectronic?

A

have the same electron count as an ion present on the periodic table

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16
Q

What is the bond definition of a non-polar covalent bond, and the physical properties it may exhibit?

A

-the bond shows two elements that are shared equally because their electronegativity rates are close in amount
-the bond is then neutral through this process

physical properties:
-soft due to weak intermolecular forces
-low melting and boiling points

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17
Q

What is the bond definition of a polar covalent bond, and the physical properties it may exhibit?

A

-made up of cations which have a positive charge, and anions which have a negative charge and when they bond they neutralize as opposites attract, the transfer of electrons to non-metals allows this to occur

physical properties:
-brittle
-high melting points and boiling points

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18
Q

What are isotopes?

A

-atoms of one element that differ by the number of neutrons in the nucleus

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19
Q

What is atomic number?

A

-the number of protons present in the nucleus of an atom
-identifies the element (different elements don’t share atomic number)
-isotopes of one element have the same atomic number

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20
Q

What is mass number?

A

-the sum of the protons and neutrons present in the nucleus of an atom
-isotopes of one element have different mass numbers *NOT THE SAME AS ATOMIC MASS
-the isotopic mass number is not found by using the periodic table

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21
Q

What are stable isotopes?

A

-isotopes that share the same physical and chemical properties

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22
Q

What are radioisotopes?

A

-unstable isotopes as they have unstable amounts of protons and neutrons
-the nucleus is destabilized
-these unstable nuclei are radioactive, and they emit radiation through particles when they attempt to re-stabilize

23
Q

What are the three types of radiation?

A

-alpha, beta, gamma

24
Q

What are the uses of radioisotopes?

A

agriculture: added to fertilizer
food preservation: slows down spoilage
medicine: disease treatment
electricity generation: nuclear power plants
archeology: carbon dating

25
Q

How do you determine the subatomic particle counts for the isotopes of atoms?

A

number of protons: atomic number
number of electrons when neutral: the same as the atomic number
number of neutrons: mass number - atomic number

26
Q

How do you represent an isotope in atomic notation?

A

mass number
X
atomic number

27
Q

How do you represent an isotope in isotopic notation?

A

X-mass number

28
Q

What is isotopic abundance?

A

-the amount of a given isotope of an element that exists in nature, expressed as a percentage of the total amount of the element
-the average atomic mass which appears on the periodic table is a weighted average that factors in the mass of all the naturally occurring stable isotopes to their percentage abundance

29
Q

What is the equation for calculating the weighted atomic mass of a naturally occurring isotope?

A

wam = (% isotope #1 x mass isotope #1) + ((% isotope #2 x mass isotope #2) +….

percentage expressed as decimal, divided by 100!

30
Q

What is the atomic radius?

A

-the approximate distance from the
centre of the nucleus to the
the approximate outer boundary of the
cloud-like region of its valence
electrons

31
Q

Describe the trend of atomic radius as you travel up and down a group

A

atomic radius INCREASES DOWN a group
WHY?
-moving down a group, each subsequent element has one additional orbit
thus the valence electrons are further away from the nucleus
-further away from the nucleus, the valence electrons experience less attractive forces from the nucleus

32
Q

Describe the trend of atomic radius as you travel from left to right across a period

A

atomic radius DECREASES ACROSS a period
WHY?
-the number of protons in the nucleus increases so the nucleus gets stronger and pulls the outer electrons closer

33
Q

What is an ionic radius?

A

the radius of the stable ion of an atom

34
Q

What is the trend when comparing a neutral atom to a stable ion?

A

cations: removal of electrons (+ charge)
-have a smaller radius than a neutral atom because there is one less orbit so the valence electrons are now closer to the nucleus

anions: adding of electrons (- charge)
-anions have a larger radius than those of a neutral atom because the nuclear charge stays the same however the gaining of electrons makes the repulsive forces increase (enlarged electron cloud)

35
Q

What is first ionization energy?

A

the energy needed to remove a valence electron from a neutral atom to form a positive charge

36
Q

What is the trend associated with the first ionization energy when you travel down a group?

A

first ionization energy decreases down a group
-attraction between the nucleus and electrons in the valence shell decreases down a group because atomic radius increases, meaning that less energy is needed to pull an electron away from the atom

37
Q

What is the trend associated with the first ionization energy when you travel across a period?

A

first ionization energy increases across a period
-attraction between the nucleus and electrons increases as the atomic radius decreases, causing more energy to be needed to remove an electron and pull it away from the nucleus

38
Q

What is electron affinity?

A

-the ease at which an atom can add a valence electron into its outer orbit to form a negatively charged ion

39
Q

What is the trend associated with electron affinity (electro negativity) when you travel down a group?

A

electronegativity decreases down a group
-since atomic radius increases down a group the attraction between the valence electrons and the nucleus decreases, thus the ability to attract electrons into its outer orbit also decreases

40
Q

What is the trend associated with electron affinity (electro negativity) when you travel across a period?

A

electronegativity increases across a period
-since atomic radius decreases across a period the attraction between the valence electrons and the nucleus is stronger, thus the ability to pull in electrons into the outer orbit and attract them increases

41
Q

What do Lewis dot symbols show?

A

-the element symbol with valence electrons represented

42
Q

What are the basics of chemical bonding?

A

chemical bonds form when atoms transfer or sharing valence electrons
-atoms bond with other atoms to achieve stability
-chemical stability is achieved when the valence shell of an atom is full, equal to the electron count of the nearest Noble Gas
-a stable valence shell is either 8 or, for a few elements, 2 electrons
-a full valence shell of electrons lowers the overall
energy of the atom and thus provides it with stability
-when atoms/ions share the same electron configuration
they are said to be isoelectronic

43
Q

What are intramolecular bonds?

A

Intramolecular bonds form between atoms within a molecule or
compound.

44
Q

What do ionic bonds consist of when they chemically bond?

A

electrons are transferred from one atom to another
-forms between a metal and a non-metal
-metal atoms easily lose electrons and become CATIONS as they are left with an overall positive charge
-nonmetal atoms easily gain electrons and become ANIONS as they
are left with an overall negative charge
-the cation and anion are strongly held together by electrostatic
forces of attraction (opposite charges attract)
-the overall bond remains neutral since the ion charges cancel
each other out
-referred to as ionic compounds made up of formula units

45
Q

What do covalent bonds consist of when they chemically bond?

A

-electron pairs are shared between two non-metals
-called molecular compounds

46
Q

What is a polar covalent bond?

A

electrons are shared unequally
-the shared electron pair spends more time closer to the atom with
the greater electronegativity (greater attraction for the electrons) causing the more electronegative atom to develop a
slightly negative charge while the less electronegative atom in the
bond is left with a slightly positive charge

47
Q

What is a non-polar covalent bond?

A

electrons are shared equally
-both atoms involved in the bond have essentially the same
electronegativity (degree of attraction for shared pair of
electrons)
-the bond is neutral

48
Q

What is electronegativity?

A

-the relative ability of an atom to attract a shared electron pair
when bonded
-the type of bond that forms between two atoms can be determined
by calculating the electronegativity difference between them
-metals have lower electronegativity as they lose electrons
-non-metals have greater electronegativity as they gain electrons

49
Q

How do you determine what bond forms between two atoms when labelling them as polar, non-polar, or ionic?

A

ELECTRONEGATIVITY SCALE
-less than 0.4 then the bond formed is nonpolar covalent

-between 0.4 to 1.7 then the bond formed is polar covalent

-greater than 1.7 then the bond formed is ionic
*however regardless of electronegativity difference if a bond
forms between a metal atom and a non-metal atom it is always ionic

50
Q

How do metal atoms achieve stability?

A

-Metal atoms achieve stability through chemical reactions with other atoms (namely non-metal atoms)
-A metal atom reacts to achieve stability by losing one or more electrons from its valence shell, resulting in the formation of a positively charged ion (CATION)

51
Q

What is metallic character?

A

-The chemical properties exhibited by metals are dependent on howeasily they lose electrons to form positively charged ions (cations)
-The easier a metal atom can lose the electrons from its valence shell
the more chemically reactive it is and the more metallic character it
has

52
Q

How do non-metal atoms achieve stability?

A

-Non-metal atoms achieve stability through chemical reactions with
other atoms (both metal and non-metal atoms)
-A non-metal atom achieves stability by gaining one or more electrons into its valence shell resulting in the formation of a negatively charged ion (ANION) or
by sharing pairs of electrons with another atom

53
Q

What is a non-metallic character?

A

-The chemical properties exhibited by non-metals are dependent on how easily they draw electrons into their valence shell either through accepting via transfer or by sharing
-The easier a non-metal atom can attract electrons into its valence shell the more chemically reactive it is and the more non-metallic character it has

Chemistry 11U - 2023 (4 decks)

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