Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry > Chem Test > Flashcards

Chem Test Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

Who created periodic law

A

Henry Mosley

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

Who created the first periodic table

A

Dimitri Mendeleev

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

What is periodic law

A

A law stating that when sorted by their atomic number, elements fall into repetitive patterns of chemical and physical properties.

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

Group

A

Colums of elements in the periodic table, elements in a group have the same number of valence electrons.

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

Period

A

Rows of elements in the periodic table. Elements in a period have the same number of electron shells.

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

Representative elements

A

Found in the s-block and p-block, these are elements that have a wide range of chemical and physical properties. Also called main group elements.

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

Transition elements

A

Found in groups 3-12. Also known as d block elements. Not as chemically reactive as s-block. Metallic elements with partially filled d orbitals.

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

Metal

A

A metal is defined by metallic properties such as being ductile, good conductors of electricity, shiny, high melting point, high density, malleable, good conductor of heat.

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

Alkali metals

A

Found in group 1 (1 valence electron). Called alkali because their reaction with water forms alkalies. Which are strong bases capable of neutralizing acid. Both Alkali and Alkaline earth metals are soft, silvery, reactive metals.

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

Lanthanides and Actinides

A

Elements in the f block. Lanthanides have properties similar properties to those in group 2 (Alkaline Earth Metals). Actinides are radioactive elements that are mostly synthetic or man made.

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

non-metal

A

an element without metallic properties

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

Valence electrons

A

electrons in the outer most shell that participate in bonding

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

core electrons

A

electrons that are not valence electrons and do not participate in bonding they are the same across a period.

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

Alkaline earth metals

A

second most reactive elements found in group 2 (2 valence electrons) Both Alkali and Alkaline earth metals are soft, silvery, reactive metals.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Halogen

A

group 17 elements (7 valence electrons) They are the most active group of non-metals. They react with metals in groups 1 and 2 to form salts. Halogen means salt maker.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Noble gasses

A

Found in group 18 (8 valence electrons) Also called inert gasses. Stable elements that don’t form compounds. have completly filled outer shells and they don’t react. They rarely form compounds.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Metalloids

A

Also called semiconductors. an element which has physical and chemical properties of a metal and nonmetal. Boron, Silicone, Germanium, Arsenic, Antimony, Tellurium, and Po.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Law of octaves

A

Created by English Chemist John Newlands that if chemical elements are arranged according to increasing atomic mass properties will repeat every 8 elements.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Bond radius

A

distance between the nucleii of two bonded atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Who was Antoine Lavosier

A

French scientist that complied a list of all known elements and organized them in four catagories.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Which elements had pre-historic orgins

A

silver, gold, carbon, and oxygen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Who was John Newlands

A

an english chemist who arranged elements by increasing atomic mass.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Did the arrangement of elements by mass work for all elements?

A

no

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Why was newlands law criticized

A

because of the word octaves

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

How did Mendeleev organize the periodic table

A

by increasing atomic mass. He also placed elements with similar properties in columns, and notices periodic patterns.

26
Q

What did Mendeleev leave in the periodic table

A

spaces for yet to be discovered elements

27
Q

Mendeleev predicted the discovery of

A

scandium, gallium, and germanium

28
Q

Who publishes a periodic table right after Mendeleev

A

Lothar Meyer

29
Q

Who was Henry Mosley

A

An english chemist who arranges periodic table by increasing atomic number thereby removing discrepancies found in Mendeleevs table.

30
Q

Mosley discovered that elements have a unique number of -, he assigns each element a - based on this.

A

Protons, atomic number

31
Q

Halogens electron configurations end in

A

p5

32
Q

What is the most and least electronegative elements

A

Fluorine is the most Francium is the least

33
Q

Noble gasses electron configurations end in - except for - which is irregular

A

p6, Helium

34
Q

Electron sheilding

A

Increases down a group, not a factor across a period. addition of energy levels.

35
Q

What does electron sheilding do

A

it interferes with attractive forces between the nucleus and the electrons. Decreases attraction.

36
Q

Nuclear charge

A

The total charge in the neucleus of all the protons. Depends on the number of protons. When more protons are added attractive force increases. Increases down a group and across a period.

37
Q

Ionization energy

A

The energy needed to remove an electron. Increases down a period decreases across a group.

38
Q

Metals have low ionization energy bc

A

they lose electrons easily

39
Q

Aufbau principal

A

fill up the lower energy levels before filling higher ones.

40
Q

Hund’s rule or the bus rule

A

Each orbital must get one electron before any receive two.

41
Q

Pauli’s exclusion principal

A

only a maximum of two electrons can be in a given orbital. One spins clockwise the other counter clockwise.

42
Q

Why are L and A pulled out of the transition elements

A

to make the table easier to read and understand.

43
Q

Why do elements in the same groups have similar chemical properties

A

because of their valence electrons

44
Q

Atomic radius

A

one half the distance between the nuclei of two bonded atoms. (Half bond length) it increases down a group and decreases across a period. Goes by Francium.

45
Q

Why does atomic radius decrease across a period

A

because of the increase in nuclear charge. It has more protons.

46
Q

Why does atomic radius increase down a group

A

additional energy levels

47
Q

Ionization energy can be based on - but there are exceptions such as -

A

distance from Fluorine (and if they’re the same distance which is higher), such as

48
Q

Why does ionization energy increase across a period

A

Atomic radius decreases, increase in nuclear charge.

49
Q

Why does ionization energy decrease down a group

A

Electron shielding (they’re further away from neucleus attraction is less easier to take off)

50
Q

Electron affinity

A

Energy required to add an electron. Increase across a period decrease down a group, again you can go by Fluorine.

51
Q

What are the electron affinity exceptions to the Fluorine rule

A

group 1 is higher than group 2; g14 is higher than g15; Halogens have a lot and Noble gasses do not.

52
Q

Why does electron affinity increase across a period

A

increase in nuclear charge

53
Q

why does electron affinity decrease down a group

A

distance increases (additional energy levels and electron sheilding)

54
Q

Electronegativity

A

how well an element attracts electrons. increase across a period decrease down a group.

55
Q

Halogens are - electronegative while noble gasses are - electronegative. This is because…

A

Very, not. This is because Halogens want another electron so they can have a full set of 8 and noble gasses dont need any more since they already have 8 and a full outer shell.

56
Q

A way to find which element is more electronegative is see

A

which is higher and closer to Fluorine

57
Q

electronegativity increases across a period because of

A

increase in nuclear charge

58
Q

Electronegativity decreases down a group because

A

distance increases (additional energy levels + electron sheilding)

59
Q

Metallic charachter

A

how closely an elements properties match that of a metal. Increase down a group decrease across a period bc you get closer to metals further from non-metals.

60
Q

Ionic radius

A

half of the distance between the neucli of two bonded ions. increase down a group decrease across a period

61
Q

why does ionic radius decrease across a period

A

increase in nuclear charge

62
Q

why does ionic radius increase down a group

A

additional energy levels

Chemistry (6 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions