Chem unit 4 Flashcards

Part 1

1
Q

First person to arrange the element by similar properties in increasing atomic mass

A

John newlands

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Who published the periodic table in 1869

A

lothar Meyer

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Who arranged to the elements by the atomic number

A

Henry Mosely

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Who published the periodic table in 1870 leaving gaps for undiscovered elements and arrange them by weight

A

Dimitri mendeleev

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Elements properties and function functions of their atomic number

A

Periodic law

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

To the left of the staircase, mostly solid at temperature except mercury

A

Metals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Group =

A

Column

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Periods =

A

Rows

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Right of staircase, liquids, and gases at room temp

A

Nonmetals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Two sides, touching staircase, except aluminum

A

Metalloids/semi conductors

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

S&P Block

A

Main group elements

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Group Except h, very reactive with water, one valence electron, soft and shiny, lower boiling point and melting point that most metals

A

Alkali metals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

, two valence electrons, harder and more dense, higher melting point in boiling point, dull in color

A

Alkali earth metals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

D&F block, wide range of properties

A

Transition metals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

4F row

A

Lathanides

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

5F row

A

Actinides

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Transition metals, Actinides and lathanides are

A

All radioactive

15
Q

very reactive with metals Which form salts (Any ionic compound that doesn’t contain h+ or OH-)

16
Q

very unreactive, full octet stable

A

Noble gases

17
Q

Group of its own

18
Q

Patterns of properties of elements

A

Periodic trend

19
Q

Tendency of an atom to attract electrons

A

Electronegativity

20
Q

Electronegativities trend

A

Increases right and up

21
Q

Reasons for electronegativities trend. L-R

A

More protons and nucleus equals greater effective nuclear charge, greater attraction for electrons

22
Reasons for electronegativities trend going up
Valence electrons get closer to the nucleus and there’s less electron shielding equals stronger pool on electrons
23
Core electrons shield, valence electrons
Electron shielding
24
Energy required to remove electrons
Ionization energy
25
Trend for ionization energy
Increases Right and up
26
Reasons for ionization trend left to right
same an EN, more protons greater effective nuclear charge = greater pool on electrons = more energy to remove electrons
27
Reasons for ionization energy bottom up
same as EN, Valence electrons are closer to nucleus and less shielding means greater on electrons and more energy to remove electrons
28
Half the distance between center of two nuclei
Atomic radius
29
Trend for atomic radius
Increases Down and left
30
Reason for trend in atomic radius right to left
Who were protons less effective nuclear charge? E/E repulsion increases meaning bigger atoms.
31
Reasons for atomic radius trend to increase going down
Valance electrons get farther from nucleus and move electrons shielding
32
Cations in atomic radius
Decrease e/e repulsion and radius decreases
33
Anions in atomic radius
Increases e/e repulsion and radius increases
34
Energy given off when an electron is added
Electron affinity
35
Trend for electron affinity
Gets more negative to the right and up
36
Reasons for electron affinity
Gives off energy equals more stable
37
Most metallic elements are lower on the periodic table
Metallic character