2014 Chapter 4 - The Periodic Table Flashcards
Electron configuration
arrangement of electrons in electron shells
Electron shells
also known as energy levels, the regions surrounding the nucleus where electrons may be found
Element
a substance composed of atoms with the same atomic number; 118 are known to exist
Energy levels
also known as electron shells, the regions surrounding the nucleus where electrons may be found
Ground state
the lowest energy arrangement of an atom’s electrons in energy levels (shells)
Indirect evidence
evidence that does not involve direct observation
Nucleus
heavy core at the centre of the atom, made of protons and neutrons
Actinides
a special block of metallic elements with atomic numbers 89-103
Groups
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
Lanthanides
a special block of metallic elements with atomic numbers 58-71
Periodic table
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
Periods
horziontal rows of the periodic table; period number of an element is equal to the number of electron shells
Transition elements
a special block of metallic elements covering elements from groups 3-12
Bonds
links that join atoms together
Covalent bonding
the sharing of electrons between atoms of non-metals
Inert gases
also known as noble gases, group 18 elements known for their stability (lack of reactivity)
Ionic bonding
attraction of positive and negative ions formed from the transfer of electrons from metallic to non-metallic atoms
Ions
“charged atoms” (or groups of atoms) formed by electrons being transferred from one atom to another
Lattices
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
Metallic bonding
a mutual attraction between a lattice of positive metal ions and a sea of delocalised, outer-shell electrons
Molecules
discrete groupings of atoms covalently bonded together
Monatomic
atoms that exist on their own, without bonding with others
Noble gases
also known as inert gases, group 18 elements known for their stability (lack of reactivity)
Alkali metals
group 1 elements
Alkaline earths
group 2 elements
Allotropes
forms of the same element that have different molecular structures and therefore different properties
Halogens
group 17 elements
Organic
compound that is or was part of a living thing; contains carbon
Organic molecules
molecules that have a backbone of carbon
Name the particles in the: a.) nucleus b.) space around the nucleus
a.) proton & neutron b.) electron
List the following in order from smallest to largest: atom, electron, proton, neutron
electron, proton, neutron, atom
A particular atom has 8 protons, 8 electrons and 9 neutrons. State its atomic number
8
State the element symbols for: a.) oxygen b.) chlorine c.) magnesium d.) iron
a.) O b.) Cl c.) Mg d.) Fe
Name the following elements: a.) F b.) Ca c.) Na d.) Pb
a.) Fluorine b.) Calcium c.) Sodium d.) Lead
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
State the number of electrons that can fit in each of the first four electron shells
2,8,18,32
State how many electrons are in an atom that has an electron configuration of 2,8,8
18
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
Explain why most of an atom’s mass is due to its nucleus
proton and neutron is about 1800 times heavier than electron
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
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
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
List the elements that Dobereiner organised into three triads
1.) Lithium, sodium, potassium 2.) Chlorine, bromine, iodine 3.) Calcium, strontium, barium
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
Name the element that was once called eka-silicon
Germanium
Explain why Mendeleev left gaps in his original table
so that incoming elements that is yet to be discovered can fill it in
Explain why Dobereiner organised selected elements into triads
because those in a triad have similar properties
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
Sodium has 11 electrons. When in its ground state, its electron configuration is…?
2,8,1
An atom has an electron configuration of 2,8,8,1. What group would it be in?
1
Covalent bonding occurs between…?
non-metal atoms and other non-metal atoms
Aluminium is in group 13 (Group III). Use this information to determine the most likely charge of aluminium ions, which is…?
+3
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
Calcium has an atomic number of 20 State how many protons would be in the nuclei of its atoms
20
Calcium has an atomic number of 20 State how many electrons would be in each of its atoms
20
Calcium has an atomic number of 20 State the electron configuration of its atoms
2,8,8,2
Calcium has an atomic number of 20 Predict the most likely charge of calcium ions
+2
Identify the period and group that these atoms would belong to. Ne
period 2, group VIII or group 18
Identify the period and group that these atoms would belong to. an atom with atomic number 13
period 3, group III or group 13
Identify the period and group that these atoms would belong to. an atom with 7 electrons
period 2, group V or group 15
Determine the electron configuration of an atom in: period 2, group 16
2,6
Determine the electron configuration of an atom in: period 3, group 18
2,8,8
Determine how many electrons in an atom: with eight protons
8
Determine how many electrons in an atom: with 18 protons
18
Determine how many electrons in an atom: with an atomic number of 3
3
Determine how many electrons in an atom: with an atomic number of 19
19
Determine how many electrons in an atom: in period 2, group 17
17
Determine how many electrons in an atom: in period 3, group 2
12
Determine how many electrons in an atom: of phosphorus
15
Determine how many electrons in an atom: of potassium
19
Write the chemical formula for ammonia
NH3
Write the chemical formula for Silicon tetrafluoride
SiF4
Write the chemical formula for Phosphorus trichloride
PCl3
Write the chemical formula for Sulfur Monoxide
SO
State whether the following elements have a high or low attraction for outer-shell electrons. a.) metals b.) non-metals
a.) low b.) high
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
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
Name the ions formed from the following atoms a.) sodium b.) chlorine c.) oxygen
a.) Na[+] ; cation b.) Cl[-] ; anion c.) O[2-] ; anion
Name two forms of carbon that are lattice structures
Graphite & diamond
Define the terms: malleable
can be bent
Define the terms: ductile
can be stretched
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
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
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
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
Which group is alkali metals?
group 1
Which group is alkaline earths?
group 2
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.
Examples of pure carbon exists in several different forms or allotropes. Name four.
amorphous carbon (charcoal), diamond, graphite, buckyballs
From top to the bottom of the periodic table, does the reactivity increase or decrease for group 17?
decrease
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
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
Name the separation method that is used to separate noble gases in the air
Distillation
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.
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.
What is the form that Silicon take so that it exists? State it in worded chemical formula.
Silicon dioxide and metal silicates
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
What is glass’ major component?
Silicon
What is the other name for amorphous carbon? State the common name.
Charcoal
What are the properties of metal?
- Malleable - Ductile - Conductors of heat - Conductors of electricity - Lustrous (shiny)
What can you use to see atoms?
- Scanning Tunnelling Microscope (STM)
What is the weakness of STM?
It cannot show the sub-particles of an atom; neutrons, protons and electrons
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
Product of acid + base
water + salt
Product of metal + acid
salt + hydrogen gas
Product of metal carbonate + acid
salt + carbon dioxide gas + water
Balance this equation
KOH(s) + H2SO4(aq) → K2SO4(aq) + H2O(g).
2KOH(s) + H2SO4(aq) → K2SO4(aq) + 2H2O(g).
