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School > Chemistry: Chapter 6 [DONE] > Flashcards

Chemistry: Chapter 6 [DONE] Flashcards

1
Q

How did chemists begin to organize the known elements?

A

they used the early properties of elements to sort them into groups

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2
Q

how did Mendeleev organize his periodic table?

A

he arranged them in order of increasing atomic mass

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3
Q

Who is J.W. Dobereiner?

What did he do? (2)

A

a German chemist, who created the classification system where elements are grouped into triads (sets of three elements according to similar properties)

noticed pattern in triads; one element in each triad tended to have properties with values that fell between the other two elements.

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4
Q

Who is Dmitri Mendeleev?

What did he do?

A

a Russian chemist, who published a table of the elements

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5
Q

Who was Lothar Meyer?

A

a German chemist, who published a nearly identical table like Mendeleev’s.

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6
Q

How did Mendeleev build his table?

What was the organization he chose to use?

A

put them each onto a note card, which allowed him to move the note cards around until he found the order he wanted to use

the organization he chose was a periodic table

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7
Q

Why did Mendeleev put spaces into his table?

A

because he predicted that elements would be discovered to fill those spaces

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8
Q

How is the modern periodic table organized?

A

the elements are arranged in order of increasing atomic number

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9
Q

What mistake did Mendeleev make?

A

he broke his rule of arranging the elements in order of atomic mass and he placed tellurium before iodine

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10
Q

When did Mendeleev develop his table of elements? (not the date)

A

Before he knew about the structure of atoms or about their protons

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11
Q

Who is Henry Moseley?

A

a British physicist, who determined an atomic number for all of the known elements

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12
Q

Periods go…?

A

horizontal

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13
Q

groups go…?

A

vertical

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14
Q

What is the pattern within the periods?

A

each period correspond to a principal energy level

ex. Period 1 = 2 elements –> 2 electrons (n=1); Period 2 = 8 elements –> 8 electrons (n=2); Period 3 = 18 elements –> 18 electrons (n=3); etc…

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15
Q

Define periodic law

A

when elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties

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16
Q

similarities within columns / groups?

A

elements with similar chemical and physical properties end up in the same group (vertical)

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17
Q

what are the three broad classes of elements?

A

metals, metalloids, non metals

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18
Q

The International Union of Pure and Applied Chemistry (IUPAC)

(2)

A
  • sets standards for chemistry

- in 1985, they proposed a new system for labeling groups in the periodic table

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19
Q

elements become less metallic as you…?

A

go across the periodic table from left to right.

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20
Q

Properties of metals (5)

  • conductors of heat and electric current?
  • type of form at room temperature?
  • malleability?
  • ductility?
A

generally good conductors of heat and electric current

a freshly clean / cut surface of a metal will have a high luster, or sheen (caused by ability to reflect light)

all metals are solids at room temperature , EXCEPT mercury (Hg)

many are ductile (can be drawn into wires)

most are malleable (can be hammered into thin sheets, without breaking)

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21
Q

Properties of non metals (6)

  • conductors of heat and electric current?
  • type of form at room temperature?
  • malleability?
  • ductility?
A

there is a greater variation in physical properties among non metals than among metals

  • most nonmetals are gases at room temperature, although some nonmetals are solids at room temperature (ex. sulfur and phosphorus)
  • Bromine - dark-red liquid at room temperature
  • tends to have opposite properties of metals
  • poor conductors of heat and electric current, aside from carbon (C)
  • solid non metals tend to be brittle (non malleable)
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22
Q

Properties of metalloids?

  • conductors of heat and electric current?
  • type of form at room temperature?
  • malleability?
  • ductility?
A
  • similar properties of nonmetals and metals
  • under certain conditions, they can behave like a metal; under different conditions, they can behave like a non metal

*** behavior can be controlled by changing the conditions

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23
Q

what information can be displayed in a periodic table?

A

symbols and names of elements

information about the structure of their atoms (protons, neutrons, and electrons)

24
Q

how can elements be classified based on electron configurations? (4)

A

noble gases, representative elements, transition metals, or inner transition metals

25
Q

define alkali metals

A

metals In group 1A

26
Q

define alkaline earth metals

A

any metal in group 2A

27
Q

define halogen

A

a nonmetal in group 7A

28
Q

define noble gas

A

an element in group 8A

the s and p sublevels of the highest occupied energy level are filled

29
Q

define representative element

A

elements in an “A” group

the s and p sublevels in the highest occupied energy level are partially filled

30
Q

define transition metal

A

one of the group B elements in which the highest occupied s sublevel and a nearby d sublevel generally contain electrons

31
Q

define inner transition metal

A

an element in the lanthanide or actinide series

the highest occupied s sublevel and nearby f sublevel of its atoms generally contain electrons

32
Q

what groups does the s block contain?

A

elements in Groups 1A and 2A and the noble gas Helium

33
Q

what groups does the p block contain?

A

elements in Groups 3A, 4A, 5A, 6A, 7A, and 8A,

excluding helium

34
Q

what does the d block contain?

A

transition metals

35
Q

How do you find an atom’s atomic radius ?

A

Find the distance between the two atoms’ nuclei and then divide that by 2.

  • only when they’re two atoms of the same element
35
Q

what does the f block contain?

A

inner transition metals

37
Q

What is the atom’s atomic radius unit?

A

Picometers in a meter

38
Q

How do ions form?

A

positive and negative ions form when electrons are transferred between atoms

39
Q

define ion

A

an atom or group of atoms that has a positive or negative charge

40
Q

why is an atom electrically neutral?

A

because they have an even number of electrons and protons.

ex. Sodium (Na) = 11 protons and electrons

41
Q

define cation

A

an ion that lost an electron, so therefore, it has a positive charge

  • it looks like…

1+, for the formation of 1 electron

42
Q

atoms of metals tend to…

A

form ions by losing one or more electrons from their highest energy levels

43
Q

define anion

A

an ion that gained an electron, so therefore, it has a negative charge

  • it looks like…

1-, for the loss of 1 electron

44
Q

atoms of nonmetals tend to…

A

form ions by gaining one or more electrons

45
Q

Ionization Energy

A

energy required to remove an electron from an atom

  • used when the element is in a gaseous state
46
Q

how do electrons move to higher energy levels ?

A

when atoms absorb energy

47
Q

what does ionization energies help you predict?

A

what ions an element will form

48
Q

define first ionization energy

A

energy required to remove the FIRST electron from an atom

49
Q

what is the product of the first ionization energy?

A

1+ (the gain of one electron)

50
Q

define electronegativity

A

the ability of an atom of an element to attract electrons when the atoms is in a compound.

51
Q

cations are always….

A

smaller than the atoms from which they form

52
Q

anions are always…

A

larger than the atoms from which they form

53
Q

Least electronegative element? what’s the value?
What does this mean?

MOST electronegative element? what’s the value?

A
  • Cesium (Ce): 0.7; least tendency to attract electrons tends to lose electrons –> formation of cations
  • Fluorine (F): 4.0; strong tendency to attract electrons tends to gain electrons –> formation of anions
54
Q

How does an atom gain / lose electrons?

A

It occurs when the bond between atoms is broken so that the shared electrons go with the element that has the higher electronegativity. (the one with the higher electronegativity will have

55
Q

Atomic Charge / Radius / Size

A
  • Within a group: size / radius increases as you go from top to bottom; the charge on the nucleus also increases and the number of occupied energy levels increase.
  • ***the increase in the nucleus’s charge draws electrons closer to the nucleus
  • *** the increase in occupied energy levels (period #’s) = increase in shielding (SHIELDING EFFECT IS GREATER THAN THE ATOMIC CHARGE, SO THE SIZE INCREASES)
  • increases from left to right and top to bottom.
  • can also tell by atomic number *bigger atomic number = more protons and electrons = bigger atom size / radius

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