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Chem > Quest > Flashcards

Quest Flashcards

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1
Q

What did Mendeleev do

A

Created periodic table by organizing elements by increasing ATOMIC MASS
Similar properties were grouped together

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2
Q

T or F, mendeleevs periodic table had some discrepancies

A

True, however he could predict properties of undiscovered elements

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3
Q

What did Henry Mosley do

A

Organized elements by INCREASING ATOMIC NUMBER in his periodic table, resolved mendeleevs discrepancies

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4
Q

Which way does a period go

A
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5
Q

Which way do columns, groups, families go

A 
^
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6
Q

Where are metals located

A

Left side besides hydrogen

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7
Q

Where are non metals located

A

Right side

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8
Q

Where are metalloids located

A

In the diagonal piece

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9
Q

Most metallic and gaseous

A

Metallic-francium

Gaseous- hydrogen

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10
Q

Increase metallic property

A 
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11
Q

Alkali metals

A

Group one

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12
Q

Alkaline earth metals

A

Group two

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13
Q

Transition metals

A

Body section

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14
Q

Halogens

A

Group next to Nobel gases

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15
Q

Nobel gases

A

Last group

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16
Q

Noble gases

A

Stable octet- full valence
Colorless gases
Monatomic-come alone very unreactive

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17
Q

Alkali earth metal

A 
One electron valence 
Very reactive 
Form ionic compounds with non metals
Form insoluble salts with silver
Diatomic (exists in pairs)
18
Q

What are gases at SATP

A

Fluorine and chlorine

19
Q

What are liquid at SATP

A

Bromine

20
Q

What are solids at SATP

A

Iodine and astatine

21
Q

T or F, SATP states can be found on chem helper

A

TRUEEEE

22
Q

Periodic law

A

When elements are arranged in order of increasing atomic number, elements with similar properties appear of regular intervals

23
Q

How is atomic radius calculated

A

Distance between two nuclei divided by two

24
Q

Cations

A

Positive.
Lose electrons
Smaller atomic radius

25
Q

Anions

A

Negative
Gain electrons
Larger atomic radius

26
Q

Atomic radius across periods and down groups

A

Across period- decreases

Down groups- increases

27
Q

Ionization across periods and down groups

A

Across periods- increases

Down groups- decreases

28
Q

Electronegativity across periods and down groups

A

Across periods- increases

Down groups- decreases

29
Q

Ionization energy

A

The energy required to remove an electron from an gaseous atom

30
Q

Why is an atom with high ionization not likely to form positive ion

A

Strong hold on electrons so it’s not likely to lose an electron

31
Q

Octet rule

A

Atoms tend to gain, lose, or share electrons in order to get a full valence outer shell

32
Q

Electronegativity

A

Atoms ability to attract electrons in a chemical bond

33
Q

What is the relationship between attractive force and number of protons and electrons

A

The attractive force of the nucleus is not divided up amount electrons of the atom, each electron gets the full attractive force of the nucleus

34
Q

Octaves

A

Properties of the elements repeated every eight elements

35
Q

Periodic law

A

When elements are arranged according to increasing atomic number, there is a periodic repetition of their chemical and physical properties

36
Q

Similar chemical properties are located

A

Down a group

37
Q

Similar chemical properties down a group because

A

They have the same number of valence electrons

38
Q

Energy level of valence electron related to period

A

Period number is the number of the energy level the valence electrons are on

39
Q

Coloumbic attraction

A

Attraction between oppositely charged particles

40
Q

Halogens

A 
Seven valence
Very reactive 
Non metals
Form ionic compounds with metals 
Diatomic
41
Q

Atomic radius
Electronegativity
Ionization trends

A

Atomic radius increases down and decreases to the right

Others are inverse

Chem (14 decks)

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