2014 Chapter 4 - The Periodic Table Flashcards
1
Q
Electron configuration
A
arrangement of electrons in electron shells
2
Q
Electron shells
A
also known as energy levels, the regions surrounding the nucleus where electrons may be found
3
Q
Element
A
a substance composed of atoms with the same atomic number; 118 are known to exist
4
Q
Energy levels
A
also known as electron shells, the regions surrounding the nucleus where electrons may be found
5
Q
Ground state
A
the lowest energy arrangement of an atom’s electrons in energy levels (shells)
6
Q
Indirect evidence
A
evidence that does not involve direct observation
7
Q
Nucleus
A
heavy core at the centre of the atom, made of protons and neutrons
8
Q
Actinides
A
a special block of metallic elements with atomic numbers 89-103
9
Q
Groups
A
vertical columns of the periodic table; group number is equal to the number of electrons in the outer shell of atoms of the elements in that group
10
Q
Lanthanides
A
a special block of metallic elements with atomic numbers 58-71
11
Q
Periodic table
A
a list of all the known elements, arranged horizontally in order of increasing atomic number and vertically according to the number of electrons in the outer shell
12
Q
Periods
A
horziontal rows of the periodic table; period number of an element is equal to the number of electron shells
13
Q
Transition elements
A
a special block of metallic elements covering elements from groups 3-12
14
Q
Bonds
A
links that join atoms together
15
Q
Covalent bonding
A
the sharing of electrons between atoms of non-metals
16
Q
Inert gases
A
also known as noble gases, group 18 elements known for their stability (lack of reactivity)
17
Q
Ionic bonding
A
attraction of positive and negative ions formed from the transfer of electrons from metallic to non-metallic atoms
18
Q
Ions
A
“charged atoms” (or groups of atoms) formed by electrons being transferred from one atom to another
19
Q
Lattices
A
a regular arrangement of particles. In ionic lattices, the particles are ions; in solid molecular lattices, the particles are molecules; and in diamond and graphite, the particles are atoms
20
Q
Metallic bonding
A
a mutual attraction between a lattice of positive metal ions and a sea of delocalised, outer-shell electrons
21
Q
Molecules
A
discrete groupings of atoms covalently bonded together
22
Q
Monatomic
A
atoms that exist on their own, without bonding with others
23
Q
Noble gases
A
also known as inert gases, group 18 elements known for their stability (lack of reactivity)
24
Q
Alkali metals
A
group 1 elements
25
Alkaline earths
group 2 elements
26
Allotropes
forms of the same element that have different molecular structures and therefore different properties
27
Halogens
group 17 elements
28
Organic
compound that is or was part of a living thing; contains carbon
29
Organic molecules
molecules that have a backbone of carbon
30
Name the particles in the: a.) nucleus b.) space around the nucleus
a.) proton & neutron b.) electron
31
List the following in order from smallest to largest: atom, electron, proton, neutron
electron, proton, neutron, atom
32
A particular atom has 8 protons, 8 electrons and 9 neutrons. State its atomic number
8
33
State the element symbols for: a.) oxygen b.) chlorine c.) magnesium d.) iron
a.) O b.) Cl c.) Mg d.) Fe
34
Name the following elements: a.) F b.) Ca c.) Na d.) Pb
a.) Fluorine b.) Calcium c.) Sodium d.) Lead
35
State the electric charge of each of: a.) a proton b.) an electron c.) a neutron d.) a nucleus e.) an atom
a.) positive b.) negative c.) neutral d.) positive e.) neutral
36
State the number of electrons that can fit in each of the first four electron shells
2,8,18,32
37
State how many electrons are in an atom that has an electron configuration of 2,8,8
18
38
Define the following terms: a.) STM b.) indirect evidence c.) atomic number
a.) Scanning Tunneling Microscope b.) evidence that is not based from direct observation c.) proton quantity
39
Explain why most of an atom's mass is due to its nucleus
proton and neutron is about 1800 times heavier than electron
40
Demonstrate how to write electron configurations by writing them for the following atoms. a.) lithium (with 3 electrons) b.) carbon (with 6 electrons) c.) sodium (with 11 electrons) d.) chlorine (with 17 electrons)
a.) 2,1 b.) 2,4 c.) 2,8,1 d.) 2,8,7
41
Compare a proton with a neutron by listing their similarities and differences
Similarities: about the same weight, in the nucleus, next to each other Differences (neutron): neutral Differences (proton): positive
42
List five: a.) group 15 elements b.) period 2 elements c.) common transition elements d.) lanthanides e.) actinides
a.) nitrogen, phosphorus, arsenic, antimony, bismuth b.) lithium, beryllium, boron, carbon, nitrogen c.) copper, gold, silver, titanium, iron d.) lanthanium, cerium, praseodynium, neodynium, promethium e.) actinium, thorium, protactinium, uranium, neptunium
43
List the elements that Dobereiner organised into three triads
1.) Lithium, sodium, potassium 2.) Chlorine, bromine, iodine 3.) Calcium, strontium, barium
44
Outline how the electron configuration of an element determines its position in the periodic table
1.) Number of integers shown determines which period it belongs to 2.) Number of electrons in its outer shells determines the group
45
Name the element that was once called eka-silicon
Germanium
46
Explain why Mendeleev left gaps in his original table
so that incoming elements that is yet to be discovered can fill it in
47
Explain why Dobereiner organised selected elements into triads
because those in a triad have similar properties
48
The electron configurations of different elements are given below. Identify in which period and group they should be placed. a.) 2,3 b.) 2,8,7 c.) 2,8,8,2 d.) 2,8,18,6 e.) 2,8,18,8,2
a.) Period 2, group 3 b.) period 3, group 7 c.) period 4, group 2 d.) period 4, group 6 e.) period 5, group 2
49
Sodium has 11 electrons. When in its ground state, its electron configuration is...?
2,8,1
50
An atom has an electron configuration of 2,8,8,1. What group would it be in?
1
51
Covalent bonding occurs between...?
non-metal atoms and other non-metal atoms
52
Aluminium is in group 13 (Group III). Use this information to determine the most likely charge of aluminium ions, which is...?
+3
53
Nitrogen N is in period 2, group 15. Which of the following elements would have properties most similar to nitrogen? A. phosphorus P (period 3, group 15) B. oxygen O (period 2, group 16) C. neon Ne (period 2, group 18) D. sodium (Na) because its symbol also starts with N
A
54
Calcium has an atomic number of 20 State how many protons would be in the nuclei of its atoms
20
55
Calcium has an atomic number of 20 State how many electrons would be in each of its atoms
20
56
Calcium has an atomic number of 20 State the electron configuration of its atoms
2,8,8,2
57
Calcium has an atomic number of 20 Predict the most likely charge of calcium ions
+2
58
Identify the period and group that these atoms would belong to. Ne
period 2, group VIII or group 18
59
Identify the period and group that these atoms would belong to. an atom with atomic number 13
period 3, group III or group 13
60
Identify the period and group that these atoms would belong to. an atom with 7 electrons
period 2, group V or group 15
61
Determine the electron configuration of an atom in: period 2, group 16
2,6
62
Determine the electron configuration of an atom in: period 3, group 18
2,8,8
63
Determine how many electrons in an atom: with eight protons
8
64
Determine how many electrons in an atom: with 18 protons
18
65
Determine how many electrons in an atom: with an atomic number of 3
3
66
Determine how many electrons in an atom: with an atomic number of 19
19
67
Determine how many electrons in an atom: in period 2, group 17
17
68
Determine how many electrons in an atom: in period 3, group 2
12
69
Determine how many electrons in an atom: of phosphorus
15
70
Determine how many electrons in an atom: of potassium
19
71
Write the chemical formula for ammonia
NH3
72
Write the chemical formula for Silicon tetrafluoride
SiF4
73
Write the chemical formula for Phosphorus trichloride
PCl3
74
Write the chemical formula for Sulfur Monoxide
SO
75
State whether the following elements have a high or low attraction for outer-shell electrons. a.) metals b.) non-metals
a.) low b.) high
76
Recall the different types of bonding by matching them with correct combination of elements. (match alphabets with numbers) a.) metallic b.) ionic c.) covalent i.) metal/non-metal ii.) non-metal/non-metal iii.) metal/metal
metallic = metal/metal ionic = metal/non-metal covalent = metal/metal
77
Recall the different types of bonding by matching them with the term that best identifies them: (match alphabets with numbers) a.) metallic b.) ionic c.) covalent i.) shared electrons ii.) electron sea iii.) charged atoms
metallic = electron sea ionic = charged atoms covalent = shared electrons
78
Name the ions formed from the following atoms a.) sodium b.) chlorine c.) oxygen
a.) Na[+] ; cation b.) Cl[-] ; anion c.) O[2-] ; anion
79
Name two forms of carbon that are lattice structures
Graphite & diamond
80
Define the terms: malleable
can be bent
81
Define the terms: ductile
can be stretched
82
Explain why molten and dissolved sodium chloride conduct electricity but solid sodium chloride doesn't
a. ) Solid has ions packed together tightly, restricting the moments of electrons
b. ) Molten lets the ions that carry electrons move freely
83
Explain why ionic substances form lattices instead of molecules
Each ion is surrounded by ions of the opposite charge, building up a three-dimensional structure called a lattice
84
Use the metallic bonding model to explain why metals don't tend to break when bent
Because the sea of electrons are holding the atoms together
85
Use the structure of diamond to explain why it is strong
a.) Because the shape of the molecule is of the tetrahedron which gives its difficulty to break b.) because it forms 4 bonds for each carbon element, the max amount of bonds an atom can make
86
Which group is alkali metals?
group 1
87
Which group is alkaline earths?
group 2
88
From top to the bottom of the periodic table, does the reactivity increase or decrease for group 1 and 2? And why?
increase; Metal atoms have a weak hold on their outer-shell electrons. As you move down a group, extra shells are added and so this hold gets even weaker. This makes the metal more unstable and more reactive.
89
Examples of pure carbon exists in several different forms or allotropes. Name four.
amorphous carbon (charcoal), diamond, graphite, buckyballs
90
From top to the bottom of the periodic table, does the reactivity increase or decrease for group 17?
decrease
91
Describe the group 17, halogens. (name 3 dot points)
a.) are not found in nature in their pure form but are found in various types of salts, including sea salt b.) all form molecules, each being made up of two atoms (F2, Cl2, Br2, and I2) c.) have coloured and posionous vapours
92
As you go down the group 18, does each of the atoms rising rate decrease or increase? (when all of these gases are pumped into balloons, from helium to the atom at the bottom of the group becomes lighter or heavier, becomes easier to rise or harder to rise into the air?)
Rising rate decrease
93
Name the separation method that is used to separate noble gases in the air
Distillation
94
Explain why helium is used instead of hydrogen in airships
Hydrogen is unstable, helium is stable (because it's a noble gas). Therefore, hydrogen is more flammable than helium.
95
All the noble gases except radon could be used in party balloons but helium is the best. Propose a reason why.
Helium is a noble gas with least amount of electrons and neutrons and protons. Therefore, it is more stable and safer and lighter.
96
What is the form that Silicon take so that it exists? State it in worded chemical formula.
Silicon dioxide and metal silicates
97
Silicon dioxide and metal silicates together make up how much percentage of Earth's crust? And what are their common form?
75%, come in the form of sand, clay, asbestos and quartz
98
What is glass' major component?
Silicon
99
What is the other name for amorphous carbon? State the common name.
Charcoal
100
What are the properties of metal?
- Malleable - Ductile - Conductors of heat - Conductors of electricity - Lustrous (shiny)
101
What can you use to see atoms?
- Scanning Tunnelling Microscope (STM)
102
What is the weakness of STM?
It cannot show the sub-particles of an atom; neutrons, protons and electrons
103
Order the sub-atomic particles by mass from heaviest to lightest and explain how much they weigh compared to each other.
Neutrons \> Protons \> Electrons Neutrons are SLIGHTLY heavier than protons Neutrons and protons are roughly 1800 times heavier than electrons
104
Product of acid + base
water + salt
105
Product of metal + acid
salt + hydrogen gas
106
Product of metal carbonate + acid
salt + carbon dioxide gas + water
107
Balance this equation
KOH(s) + H2SO4(aq) → K2SO4(aq) + H2O(g).
2KOH(s) + H2SO4(aq) → K2SO4(aq) + 2H2O(g).
108
