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Chem 1 Scottsboro High > Unit 3 🖊️ > Flashcards

Unit 3 🖊️ Flashcards

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1
Q

What people classified the periodic table using atomic mass?

A

Dobenreigner, Mendeleev, Newlands

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2
Q

Who classified the periodic table using atomic number?

A

Mosely

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3
Q

Describe the relationship between electron configuration and the groups and columns of the periodic table

A

Elements in the same group have the same number of electrons in their outermost shell, leading to similar valence shell electronic configuration

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4
Q

What is the Atomic Radius trend?

A

1/2 distance between the nuclei of 2 atoms of the same element.
Smallest: He
Largest: Fr

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5
Q

What is the Electronegativity trend?

A

The ability of an atom to attract electrons (not including Noble Gases)
Smallest: Fr
Largest: F

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6
Q

What is the Ionization Energy trend?

A

The energy required to remove an electron from an atom
Smallest: Fr
Largest: He

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7
Q

What is the Ionic Radius trend?

A

1/2 distance between the nuclei of charged atoms; Cation<Parent<Anion
Smallest: (+) charge
Largest: (-) charge

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8
Q

Describe Electron Affinity

A

Energy needed to add an electron to a neutral atom (opposite of Ionization Energy)

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9
Q

Describe the Electron Shielding Effect

A

As you go down a group, energy levels are filled with e- generating a (-) charge shield from the nucleus

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10
Q

Describe Effective Nuclear Charge

A

As you go from left to right across the periodic table, the more protons in the nucleus; cause electrons to pair up in orbitals

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11
Q

Who believed that physical and chemical properties repeated in an orderly way

A

Mendeleev

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12
Q

Who discovered the periodic law?

A

Mosely

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13
Q

who’s periodic table was meant to show electron configurations?

A

Mosely

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14
Q

What elements did Mendeleev predict?

A

Gallium, Scandium, and Germanium

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15
Q

Who suggested that the properties of an element are related to its atomic mass?

A

Dobenreigner

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16
Q

Who classified elements into triads?

A

Dobenreigner

17
Q

How many valence electrons are in each main group of the periodic table?

A

Alkali metals: 1
Alkali Earth metals: 2
Transition metals: 1-2
Group 13: 3
Group 14: 4
Pnictogens: 5
Chalcogens: 6
Halogens: 7
Noble gases: 8

18
Q

reacts vigorously with H20

A

Alkali Metals

19
Q

Reacts vigorously with O

A

Alkali Earth metals

20
Q

What group has -4 or +4 charges; -3 charges?

A
  1. Group 14
  2. Pnictogens
21
Q

What Periodic group is used as catalysts in petroleum production?

A

Lanthanides and Actinides

22
Q

What periodic table group is mostly non-reactive?

A

Transition Metals

23
Q

What periodic group is used as catalysts?

A

Transition metals

24
Q

What periodic group was formed by accident?

A

Chalcogens

25
Q

Inert

A

Noble Gases

26
Q

Form acidic compounds

A

Halogens

27
Q

Define Valence Electrons

A

Electrons in the outermost shell of an atom that can be lost, gained, or shared (S and P orbitals only)

28
Q

What block is each group a part of?

A

Alkali Metals- s
Alkali Earth Metals- s
Transition Metals- d
Group 13- p
Group 14-p
Pnictogens- p
Chalcogens- p
Halogens- p
Noble Gases- p

29
Q

What is a periodic trend

A

Specific patterns that are present in the periodic table that illustrate different aspects of a certain element including its size and electronic properties.

30
Q

Explain why atoms form chemical bonds and distinguish between ionic and covalent bonding

A
  1. Chemical bonds happen because every atom wants to be stable; many atoms become stable by having 8 electrons or filling their valence shell with electrons
    Covalent- electrons are SHARED
    Ionic- electrons are completely TRANSFERRED
31
Q

As you go down a group on the periodic table, atoms get what?

A

Bigger

32
Q

True or false: the electron shield is generated as you go down the groups of the periodic table

A

TRUE

33
Q

The nuclear effect means…

A

The greater p+ in the nucleus, the more electrons will pair up in orbitals

34
Q

Describe cations and anions

A

A cation has a net positive electrical charge, which means it has more protons than electrons.
An anion has a net negative electrical charge, which means it has more electrons than protons. ANIONS ARE ALWAYS LARGER THAN CATIONS

35
Q

Positive or negative: Cation

A

Positive

36
Q

Positive or negative: Anion

A

Negative

37
Q

Why is Helium smaller than Hydrogen?

A

electron configuration. Helium holds electrons closer to the nucleus.

Chem 1 Scottsboro High (1 decks)

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