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Chemistry > Atomic Structure- the atom + periodic table > Flashcards

Atomic Structure- the atom + periodic table Flashcards

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1
Q
  • What are the subatomic particles?
  • What are the charges of each?
  • Which ones have similar masses?
  • Where are each located inside of an atom?
A
  • protons (+), neutrons (neutral), electrons (- charge)
  • protons and neutrons have similar masses
  • nucleus: protons + neutrons ; electron shells/ levels orbitals: electrons
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2
Q

Which subatomic particles contribute to the atomic mass/ weight?

A

protons and neutrons

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3
Q

Which subatomic particles contribute to charge of an ion?

A
  • protons (+)
  • electrons (-)
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4
Q

What is the charge of the nucleus of an atom?

A

+ bc protons + neutrons

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5
Q

Where are the orbitals located in an atom?

A

in the energy levels/ shells

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6
Q

Describe an atom (3)

A
  • mostly empty space
  • part of matter that uniquely defines an element
  • most basic complete unit of an element
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7
Q

Describe an element (3)

A
  • made up of 1 or 2 atoms
  • most basic type of matter
  • characterized by the number of protons = atomic #
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8
Q

What does the atomic # of an element represent?

A

number of protons

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9
Q

What is the # of protons stand for in an element?

A

atomic #

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10
Q

In a neutral atom/element, what 2 subatomic particles are the same in #?

A

protons and electrons, so that there is a net charge of 0.

can look at ipad the atom notes for 2 practice questions

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11
Q

What is the atomic weight/ mass of an element?

A

average # of protons + neutrons of all the isotopes of an element

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12
Q

What is the mass # if an element?

A

number of protons + # of neutrons [whole number version of atomic mass, rounded up]

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13
Q

How do you calculate the number of neutrons of an element?

A

mass # - # of protons

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14
Q

What is regular notation?
What is another name for this?

A
  • mass #, element, atomic #
  • elemental symbal
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15
Q

What is an isotope (3)?

A
  • different forms of an atom/ element
  • SAME number of protons BUT DIFFERENT number of neutrons, so different mass # as well
  • can be stable or radioactive (decaying)
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16
Q

What is the isotope notation?

A

mass #, element, atomic # OR element- mass #

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17
Q

Carbon
* valence electrons?
* atomic #?
* atomic mass?

A
  • 4
  • 6
  • 12
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18
Q

H
* valence electrons?
* atomic #?
* atomic mass?

A
  • 1
  • 1
  • 1
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19
Q

O
* valence electrons?
* atomic #?
* atomic mass?

A
  • 6
  • 8
  • 15.9 , so about 16
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20
Q

What makes up a molecule?
What are the 2 types? Describe.

A
  • 2 or more atoms

2 types
* if same atoms in the natural form, makes the diatomic elements (Have No Fear Of Ice Cold Beer)
* if different atoms, makes compounds (ie. NaCl, NH3, HCl, H2O, CO2)

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21
Q

What are ions (2) including same what and different what?

A
  • an atom or group of atoms (polyatomic ions) that HAVE A CHARGE.
  • have the SAME number of protons, BUT DIFFERENT number of electrons
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22
Q

Ions

  • What are the two types of ions?
  • Are they negative or positive? Why (ie. more or less protons/ electrons than the other)?
  • How are they formed? What type of substance forms them?
A
  • cations- postive (so more protons than electrons), form from the loss of e-‘s (to get full valence shell) by the metals
  • anions- negative (so more electrons than protons), form from the gain of e-‘s (to get full valence shell) by the nonmetals

practice questions in ipad the atom doc.

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23
Q

List the atomic structure in order (4 things)

A

subatomic particle –> atom –> element –> molecule

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24
Q

Istotopes always have the same number of _ and different number of __

A

protons; neutrons (and so diff mass #)

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25
Q

Ions always have the same number of _ and different number of __

A

protons; electrons

26
Q

How do you find the atomic mass of an atom/ element?

A

number of protons + number of neutrons

27
Q

How do you find the charge of an atom/ element?

A

protons + electrons

28
Q

The number of valence electrons in an atom/ element means the number of ___ that can be made?

A

bonds

in reality, the number of bonds an atom can form is based on the number preceding in the ionic charge a neutral atom would form

29
Q

Neutral elements with more than 4 valence e’s (ie. 5, 6, 7), what do these elements do to form an ion?

A

lots of valence electrons, so will gain more e-‘s (become anions) to form a full valence shell to become like its nearest noble gas

30
Q

Neutral elements with 4 valence e-‘s and less (so 3,2,1), what do these elements do to form ions?

A

low number of valence eletrons, so will lose electrons (become cations) to get a full valence shell. to become likes its nearest noble gas

31
Q

Generally, where do the metals lay on the periodic table

A
  • left side
  • EXCEPTION: hydrogen is actually a NON-metal
32
Q

Describe metals
* what type of ion do they tend to make and why?
* give 6 other characteristics
* what are ones i need to memorize?/ What are the valence electron numbers of those?

A
  • cations , which is from metals losing electrons bc there are few electrons in the outer/valence shell to begin with

Other characteristics
* shiny metallic luster
* GREAT heat and electrical conductors
* ductile (can be compressed into a thin wire)
* malleable (flexible, so can be hammered into different shapes without breaking)
* high density
* high melting and boiling point

Examples
* H, Na, K- 1 valence electron
* Ca, Mg - 2 valence electrons

33
Q

Generally, where do the nonmetals lay on the periodic table?

A

right side

34
Q

Describe NON-metals
* what type of ion do they tend to make and why?
* give 5 other characteristics
* what are ones i need to memorize?/ What are the valence electron numbers of those?

A
  • anions, which means nonmetals tend to gain electrons bc their outer/ valence shell has lots of electrons to begin with (so dont want to lose em)

Characteristics
* dull appearance
* POOR heat and electrical conductors
* brittle - break easily
* low density
* low melting and boiling point

Examples
* 4, 5, 6, 7 valence electrons (CNOF) (PSCl)

35
Q

Where are metalloids normally found on the periodic table?

A

starts at boron and staircases down

36
Q

Describe metalloids

A
  • can form cations or anions through loss of electrons or gain of electrons
  • have both metal and nonmetal properties
37
Q

The periodic table is arranged from L to R in order of what?

A

lowest atomic # (# of protons) [H] to the highest atomic # (# of protons) [Og]

38
Q
  • What is anothe name for the columns of the periodic table?
  • What are 2 characteristics of these columns (ie. what do they tell you)?
A
  • groups
  • the elements in the same column share similar chemical properties
  • tells use the number of valence electrons of the elements (max is 8) [EXCLUDING the transition metals]
39
Q
  • What is another name for the rows in the periodic table?
  • What do the rows tell you?
A
  • periods
  • tells us the number of energy levels/ shells (orbitals are in the levels/shells)
40
Q

What are the 4 diff orbital shapes? How many electrons can each shape hold?

A
  • spdf
  • s= 2; p= 6; d= 10; f= 14
41
Q

What are the nature of oxides of metals, nonmetals, and metalloids?

A
  • basic, acidic, and both, respectively
42
Q

What general letter group are the main group elements? transition metals?

A
  • A
  • B
43
Q

What are the 4 big groups the periodic table main group elements are grouped into ?

A
  • alkali metals
  • alkali earth metals
  • halogens
  • noble gases
44
Q

Reactivity of the periodic table ___ from left to right bc ___

A
  • decrease
  • we want to gain or lose electrons to get to a full 8 valence shell bc that is the ULTIMATE stability
45
Q

Describe alkali metals (charges they form and reactivity)

A
  • form +1 charge
  • highly reactive bc very close to becoming like a noble gas
46
Q

Describe alkali earth metals (charges they form and reactivity)

A
  • form a +2 charge
  • highly reactive BUT not as reactive as alkali metals
47
Q

Describe noble gases (charges they form and reactivity and 4 other characteristics). What is another name for them?

What ARE the noble gases?

A
  • aka inert gases
  • NON-reactive and the most stable bc they NATURALLY already have a full 8 valence shell. [ EXCEPTION: He, which has only 2 valence electrons bc only has 2 total electrons]
  • low EN, low boiling point, odorless, colorless
  • Helium, Neon, Argon, Kryton, Xenon, Radon
48
Q

Describe halogens (charges they form and reactivity and 2 other characterisitcs). What type of elements do they form?

A
  • form a -1 charge
  • highly reactive bc very close to becoming like a noble gas
  • high EN, toxic
  • diatomic elements
49
Q

neutral elements ___ electrons to form ___ and __ electrons to form ___ in order to do what?

A
  • gain, anions
  • lose, cations
  • get a full 8 valence shell to become likes its nearest noble gas
50
Q

What in general are the five periodic table trends?

A
  • ionic charge
  • atomic radii
  • ionic radii
  • ionization energy
  • electronegativity
51
Q

Describe ionic charges periodic table trend

A

in ipad

52
Q

Describe the atomic radii periodic table trend

A

in ipad

53
Q

Describe the ionic radii periodic table trend

A

in ipad

54
Q

Describe the ionization energy periodic table trend

A

in ipad

55
Q

Describe the electronegativity periodic table trend

A

in ipad

practice questions in ipad

56
Q

What is the most EN atom?

A

fluorine- in the top right of periodic table

57
Q

What atom has the largest atomic radii

A

Fr- in the lower left corner of periodic table

58
Q

What type of atoms DO NOT participate in electronegativty?

A

noble gases bc already naturally have a full valence shell of 8 electrons.

59
Q

What atom has the lowest atomic number? highest atomic number?

A
  • lowest: hydrogen
  • highest: Og
60
Q

Atoms/ elements with 1, 2, 3, or 4 valence electrons will become what type of ion?

A
  • cations (1+, 2+, 3+, 4+) –> more protons than electrons from losing electrons (bc less electrons in valence shell to begin with) to get a full valence shell of 8 to become likes its nearest noble gas
61
Q

Atoms/ elements with 5, 6, or 7 valence electrons will become what type of ion?

A

anions (-3, -2, -1) –> more electrons than protons from gaining electrons (bc more electrons in valence shell to begin with so instead of losing them will gain) to get a full valence shell of 8 to become like its nearest noble gas

Chemistry (12 decks)

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