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chemistry 2022 flashcards > the periodic table > Flashcards

the periodic table Flashcards

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1
Q

Elements are _____ and made up of ____ type of atom

A

unique

one

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2
Q

How many known elements are there?

A

118

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3
Q

What explains the differences in the physical properties of matter?

A

elements can have different numbers of protons and electrons

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4
Q

Elements can exist in different _____

A

states

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5
Q

Who invented the periodic table?

A

Dmitri Mendeleev

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6
Q

What does atomic number mean? What does it define?

A

the number of protons in the element

defines which element it is

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7
Q

What are the 3 major categories of elements based on properties?

A

Metals, metalloids, and nonmetals

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8
Q

What is atomic mass?

A

the average mass of a typical atom of a specific element (weighted for most common mass)

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9
Q

What is a row on the periodic table? What property do all elements in the same row have?

A

A period (all elements have the same # of electron shells)

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10
Q

What is a column on the periodic table? What property do all elements in the same column have?

A

A group/family (all elements have the same number of valence electrons)

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11
Q

Elements on the periodic table are arranged left to right by ______

A

increasing atomic number

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12
Q

What is a neutral atom?

A

An atom where the number of protons is the same as the number of neutrons

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13
Q

An atomic number tells you what about a neutral atom?

A

Both the number of protons and the number of electrons

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14
Q

How do you find the number of neutrons in the most common isotope with the atomic mass number and atomic number? Why does this work?

A

Subtract the atomic number from the (rounded to the nearest whole number) atomic mass number.
The atomic mass number is equal to the number of protons + the number of neutrons

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15
Q

What is an isotope? What is special about an isotope?

A

An atom of an element that has a different number of neutrons.
The number of protons is the same but the atomic mass number changes because more or less neutrons changes the mass

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16
Q

What is a mass number for an isotope?

A

The mass for an isotope of an element based on the number of protons and the number of neutrons added together.

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17
Q

What are the three isotopes of hydrogen? What makes them all different?

A

Protium (which has no neutrons), Deuterium (which has 1 neutron), and Tritium (which has 2 neutrons)

Remember that the name correlates with the mass number for these - deu=2 and tri=3, and you can figure out pro from context

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18
Q

What is an atom with a charge called?

A

An ion

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19
Q

What is a negatively charged ion called?

A

An anion

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20
Q

What is a positively charged ion called?

A

A cation

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21
Q

What are the rules for ion attraction? (2)

A

Like repels like

opposites attract

22
Q

What are some properties of metals? (6)

A
  • solid at room temp except for mercury
  • ductile (can be pulled into thin wires)
  • lustrous
  • good conductors heat and electricity
  • malleable (can be hammered into thin sheets)
  • prone to lose electrons easily
23
Q

What are some properties of nonmetals? (5)

A
  • brittle
  • dull/not shiny
  • poor conductors of heat and electricity
  • solid, liquid, or gas at room temp
  • gain or share electrons easily
24
Q

What are some properties of metalloids? (4)

A
  • nonmetallic chemical properties and metallic physical properties
  • conductivity depends
  • dull or shiny
  • solid at room temp
25
Q

What are valence electrons? What do they determine?

A

The electrons in the outermost shell of the atom.

Determine how an element reacts

26
Q

typically, most elements but hydrogen and helium want to have ___ valence electrons

A

8

27
Q

What are the 5 major groups in the periodic table?

A

Alkali metals, Alkaline Earth metals, Transition metals, Halogens, Noble Gases

28
Q

What are some properties of alkali metals? (4)

A
  • 1 valence electron
  • soft, shiny, metallic solid
  • good conductors
  • low densities and low melting points
29
Q

What are some properties of alkaline earth metals? (3)

A
  • 2 valence electron
  • metallic solids, harder than alkali metal
  • more dense, have higher melting point, better at conducting than alkali metals
30
Q

What are some properties of transition metals? (3)

A
  • hard metallic solids
  • very good conductors w/ high melting points
  • shiny, dense, lustrous
31
Q

What are some properties of halogens? (3)

A
  • 7 valence electrons
  • reactive nonmetal
  • melting and boiling points increase as atomic # increases
32
Q

What are some properties of noble gases? (2)

A
  • 8 valence electrons

- dont react often

33
Q

What are the Actinides?

A
  • mostly man made elements (except uranium and plutonium)

- 89-103

34
Q

What are the Lanthanides?

A
  • rare earth metals
  • properties all similar to first element, lanthanide
  • 57-71
35
Q

What is effective nuclear charge?

A

The total positive charge that an electron feels in an atom that has multiple electrons

36
Q

Why does effective nuclear charge matter?

A

In an electron with more than one electron, positive charge is distributed among the electrons. The full positive pull is not felt by one electron.

37
Q

Electrons in ______ (which are _____) don’t get as much positive pull as electrons in _______ (which are ____)

A

higher energy levels
farther away from the nucleus
lower energy levels
closer to the nucleus

38
Q

What is the shielding effect?

A

The balance of an electron’s attraction towards the positive nucleus and repelling from the other negative electrons in lower energy levels

39
Q

What is the atomic radius? What is its periodic trend? Why does it follow said periodic trend?

A

The distance from the center of the nucleus to the outermost electron.
right to left increase, top to bottom increase
(ex: ognesson has the highest atomic radius)
because effective nuclear charge increases as electrons are added, because there are more electrons in energy levels (respectively)

40
Q

What is ionic radius? What is its periodic trend?

A

The distance between the centers of two ions that barely touch
increases for nonmetals moving left to right across a row, increases for metals moving right to left across a row

41
Q

What is ionization energy? What is its periodic trend?

A

Ionization energy is the amount of energy/how much energy is needed to remove an electron from an atom.
increases bottom to top
increases left to right

42
Q

What is electronegativity? What is its periodic trend?

A

Electronegativity is the tendency of an atom to react.
Increases bottom to top
increases left to right
excludes the noble gases

43
Q

What are the reactivity trends for metals?

A

increasing top to bottom

increasing right to left

44
Q

What are the reactivity trends for nonmetals?

A

increasing bottom to top

increases left to right

45
Q

What are energy levels?

A

Orbits for electrons around the nucleus

46
Q

What does the Heisenburg Uncertainty Principle state?

A

it’s impossible to know both how fast a particle is going and where it is at the same time

47
Q

What does the Heisenburg Uncertainty Principle disprove? What is there instead?

A

The theory of structured orbits/circular paths around the nucleus for electrons.
Instead “orbits” are general areas of space where the electron can be located, rather than well defined paths

48
Q

What is Shrodinger’s equation the basis for?

A

Quantum mechanics, or the science of the interaction of atoms and subatomic particles (electrons, neutrons, protons, etc)

49
Q

What’s some important things to know about Schrodinger’s equation?

A
  • included both wave and particle behavior
  • say that the probability of finding an electron in a specific place is proportional to the square of the wave function
  • most likely to find a photon where the intensity of light is the highest
50
Q

What does Schrodinger’s equation tell you?

A

tells you the PROBABILITY of where the electron is at any given time
(NOT where it is)

chemistry 2022 flashcards (28 decks)

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